











































































































































































































































































































































































































































































































































































































































































































































































































































































































































































































* 

I 

.> 


/ 




Class 

Book _ M 5^2. . 
Gcpightlf_ \ Q 7.^ 

COPYRIGHT DEPOSIT* 













EXPERIMENTS IN 
PRACTICAL CHEMISTRY 

TO ACCOMPANY 

NEWELL’S PRACTICAL CHEMISTRY 


BY 

LYMAN C. NEWELL, Ph.D. (johns hopkins) 

PROFESSOR OF CHEMISTRY, BOSTON UNIVERSITY, BOSTON, MASS. 

AUTHOR OF 

“EXPERIMENTAL CHEMISTRY,” “DESCRIPTIVE CHEMISTRY,” “GENERAL 
CHEMISTRY,” “INORGANIC CHEMISTRY FOR COLLEGES,” “LABO¬ 
RATORY MANUAL OF INORGANIC CHEMISTRY,” “COLLEGE 
CHEMISTRY,” “EXPERIMENTS IN COLLEGE CHEMISTRY,” 

“PRACTICAL CHEMISTRY,” “brief COURSE IN 
CHEMISTRY,” “LABORATORY EXERCISES FOR 
A BRIEF COURSE IN CHEMISTRY” 


REVISED EDITION 


Part II 



D. C. HEATH AND COMPANY 

BOSTON NEW YORK CHICAGO 

ATLANTA SAN ERANCISCO DALLAS 

LONDON 

i?**- I?8 '*■ 







This book is the experimental part of the author’s textbook entitled 
Practical Chemistry. 

These experiments are essential for teaching the fundamental facts and 
principles of chemistry. Many practical experiments are included. 

The experiments vary in length, difficulty, and application. There are 
more experiments than a class can do in a year of chemistry. Teachers 
should select experiments which provide a course adapted to their require¬ 
ments. Ample material is available for different courses — practical, fun¬ 
damental with practical applications, college preparatory, short, and long. 

The directions for performing the early experiments are rather full. In 
the quantitative experiments, besides detailed directions, the object is stated 
and the calculation is indicated or illustrated. 

The apparatus for the pupil’s experiments is simple. Many parts are 
interchangeable, and several types of apparatus are shown. The quantities 
of chemicals have been carefully chosen, and, as a rule, the chemicals are the 
less expensive ones. The Appendix contains lists of apparatus and chem¬ 
icals. 

The Demonstration Experiments are intended for use in the class¬ 
room. The apparatus for these experiments is in List C in the Appendix. 

The Introduction contains general laboratory directions. The direc¬ 
tions for weighing (§ 8) are given in detail. 

The author is indebted to many teachers for advice, especially to his as¬ 
sociates in the chemistry department of Boston University. He is under 
special obligation to Mr. Harold C. Spencer, Boston University, 1914, for 
making the drawings. 

L. C. N. 

January, 1923 


PREFACE TO REVISED EDITION 

Several experiments have been revised and minor corrections made in 
this edition. 

L. C. N. 

April, 1929 

Copyright, 1923, 1929, 

By Lyman C. Newell. 

2H9 

Printed in U. S. A. 

OCT 11 I9?9 


©CIA 14099 


CONTENTS 


Numbers indicate experiments. College preparatory experiments are 
marked (C) — (C*) recommended, demonstration experiments (D), and 
quantitative experiments (Q). 

PAGE 

Introduction .i 

General directions — Bunsen burner — Cutting and bending 
glass tubing — Filtering — Constructing and arranging appa¬ 
ratus — Pouring liquids and transferring solids — Collecting 
gases — Weighing — Measuring — Smelling and tasting — 
Accidents 

Chemical Change — Compounds — Elements . . .13 

1. Chemical Change (C) — 2. Properties and Chemical Change 
(C*) —3. Mixture and Compound (C) — 4. Compound and 
Elements (C*) 

Oxygen.16 

5. Preparation (Short) — 6. Preparation and Properties (C*) 

— 7. Oxidation of Copper (C) — 8. Heating a Metal in Air 
(C*) (Q)—9. Rapid and Slow Oxidation (D) — 10. Air and 
Combustion (C*) 

Carbon — Carbon Dioxide — Carbon Monoxide . . 22 

n. Distribution of Carbon (C) — 12. Combustion and Carbon 
Dioxide (C) —13. Fermentation and Carbon Dioxide (C*) 

(D) — 14. Preparation and Properties of Carbon Dioxide (C*) 

— 15. Beverages and Carbon Dioxide (D) — 16. Plants and 
Carbon Dioxide (D) —17. Fire Extinguishers and Carbon 
Dioxide (D) — 18. Carbon Monoxide (D) 

Hydrogen.. . . .29 

19 Preparation (Short) (C) — 20. Preparation and Properties 
(C*) — 21. Water and Sodium (C*) (D) — 22. Burning (D) 

— 23. Reduction of Copper Oxide (C*) 

Measurement of Gases.35 

24. Weight of a Liter of Oxygen (C*) (Q) 


111 





IV 


CONTENTS 


PAGE 

Water — Hydrogen Peroxide.37 

25. In Food—26. Purification — 27. Distillation (C) — 

28. Distillation (C) (D) — 29. Physical Properties (C) — 30. 

Water Vapor and Steam (C) (D) —31. Water Vapor and Pres¬ 
sure (D) — 32. Chemical Properties (C) — 33. Solubility of Gases 
(C*) — 34. Solubility of Liquids (C*) — 35. Solubility of Solids 
(C*) — 36. Heat and Solubility (C*) — 37. Shape and Sol¬ 
ubility (C*) —38. Saturated Solutions (C*) — 39. Solubility of a 
Given Solid (C) (Q) — 40. Crystals (C) — 41. Water of Crystal¬ 
lization (C*) — 42. Crystallized Copper Sulphate (C*) (Q) —- 
43. Anhydrous Compounds (C) — 44. Efflorescence (C) — 

45. Deliquescence (C) — 46. Efflorescence and Deliquescence 
(D) — 47. Supersaturation (C) — 48. Qualitative Composition 
(D) — 49. Electrolysis (D) — 50. Hydrogen Peroxide 


Laws of Constant Composition and Multiple Proportions 52 
51. Constant Composition (C) (Q) — 52. Multiple Propor¬ 
tions (C) (Q) 

Nitrogen — Air ..56 


53. Preparation and Properties of Nitrogen (C) — 54. Nitrogen 
and Ammonia — 55. Per Cent of Oxygen in Air (C*) (Q) — 

56. Water Vapor in Air — 57. Carbon Dioxide in Air (C*)— - 

58. Testing Air 

Chlorine — Hydrogen Chloride — Hydrochloric Acid . 60 

59. Preparation and Properties of Chlorine (Short) (C*) — 

60. Preparation and Properties of Chlorine (Long) (C*) — 

61. Electrolysis of Sodium Chloride (D) — 62. Chlorine Water 
— 63. Bleaching (C) — 64. Hydrogen Chloride (C*) —- 
65. Hydrogen Chloride and Hydrochloric Acid (C*) — 66. 

Tests (C) — 67. Aqua Regia — 68. Insoluble Chlorides (C*) 

Acids, Bases, and Salts — Neutralization ... 67 

69. Acids (C) — 70. Bases (C) — 71. Salts (C)—-72. Com¬ 
position — 73. Testing for Acids and Basis — 74. Neutraliza¬ 
tion (C*) — 75. Neutralization (C*) (Q) — 76. Preparation 
of a Salt (C*) 

Ammonia — Ammonium Compounds.72 

77. Ammonia and Ammonium Hydroxide (C*) — 78. Am¬ 
monia — 79. Ammonium Salts — 80. Testing Salts (Review) 

(C) 



CONTENTS 


v 


v PAGE 

Nitric Acid — Nitrates — Nitrogen Oxides 75 

81. Nitric Acid (C*) — 82. Nitrates (C) — 83. Nitric Acid 
and Metals (C*) — 84. Test for Nitric Acid and Nitrates (C) — 

85. Nitric Oxide and Nitrogen Dioxide (C*) — 86. Nitrous 


Oxide (C*) 

Molecular Weights.80 

87. Weight of 22.4 Liters of Carbon Dioxide (C) (Q) 

Equivalent Weights.82 

88. Zinc (to Hydrogen) (C*) (Q) — 89. Magnesium (C*) 

(Q) — 90- Aluminium (C) (Q) — 91. Calcium (C) — 92. Zinc 
(to Oxygen) (C*) (Q) — 93. Zinc (to Chlorine) (C*) (Q) 

Ions and Ionization . . . . . . . .8 7 


94. Electrolytes and Non-electrolytes (C) (D) — 95. Chemi¬ 
cal Behavior of Salts (C) —■ 96. Electrolysis of Copper Sul¬ 
phate (Short) (D) — 97. Electrolysis of Copper Sulphate 
(Long) (D) — 98. Electrolysis of Sodium Sulphate (D) — 

99. Electrolysis of Potassium Iodide (D) — 100. Effect of Dis¬ 
solved Substance on the Boiling Point (C*) — 101. Effect of 
Dissolved Substance on the Freezing Point (C*) — 102. Col¬ 
ored and Colorless Ions (C) — 103. Ionization and Concen¬ 
tration (D). 

Sulphur — Hydrogen Sulphide — Sulphides ... 93 

104. Physical Properties — 105. Chemical Properties — 106. 
Orthorhombic (Rhombic) (C*) — 107. Monoclinic (C*) —- 
ic8. Amorphous (C*) —109. Hydrogen Sulphide-(Short) (C*) 

— no. Hydrogen Sulphide (Long) (C*) — in. Sulphides (C*) 

Sulphur Dioxide — Sulphurous and Sulphuric Acids — 

Salts.98 

112. Sulphur Dioxide (C*) —-113. Sulphur Dioxide and Sul¬ 
phurous Acid (C*) — 114. Sulphuric Acid (C) — 115. Tests (C) 

Carbon — Carbonic Acid — Carbonates — Oxides . . 102 

116. Graphite (C*) — 117. Charcoal (C*) — 118. Testing for 
Carbon (C) — 119. Reduction by Carbon (C) — 120. Car¬ 
bonic Acid (D) — 121. Carbonates (D) — 122. Testing for 
Carbonates—123. Carbon Monoxide (C*) (D) 

Fuels — Illuminating Gas — Flame.106 

124. Composition—125. Analysis of Coal (Q) — 126. Gaso¬ 
lene (C)—127. Kerosene —128. Davy Safety Lamp 
(C) — 129. Coal Gas — 130. Testing Illuminating Gas — 




VI 


CONTENTS 


page 

131. Gas Flame— 132. Candle Flame—133. Bunsen Burner 
and Flame (C) —134. Reduction and Oxidation with the 
Blowpipe (C) — 135. Testing for Metals and Non-metals 

Other Carbon Compounds.116 

136. Sucrose and Dextrose — 137. Starch — 138. Detection 
of Starch by Iodine — 139. Ethyl Alcohol — 140. Tests for 
Ethyl Alcohol — 141. Acetic Acid — 142. Tests for Acetic 
Acid and Acetates (C*) — 143. Vinegar—144. Preparation 
of Soap (C*) — 145. Properties of Soap (C) — 146. Carbon 
Tetrachloride 

Food and Nutrition.120 

147. Nutrients -— 148. Water —- 149. Mineral Matter — 

150. Bread — 151. Butter and Substitutes — 152. Milk (C*) 

— 153. Baking Powders (C) 

Silicon.125 

154. Sodium Silicate — 155. Silicic Acid —156. Test for 
Silicon — 157. Carborundum 

Fluorine — Bromine — Iodine. 127 

158. Etching —159. Bromine (C*)—160. Bromides (C) 

— 161. Iodine (C*) — 162. Tests for Free Iodine (C) — 

163. Iodides -(C) — 164. Halogen Acids (C*) 

Phosphates — Arsenic — Antimony — Bismuth . . .131 

165. Orthophosphoric Acid and Orthophosphates (C) — 

166. Phosphate Fertilizer — 167. Test for Arsenic (C*) — 168. 

Test for Antimony (C*) — 169. Test for Bismuth — 170. 

Fusible Alloys 

Sodium — Potassium .132 

171. Sodium (C*) — 172. Tests for Sodium (C) — 

173. Sodium Chloride (C) — 174. Sodium Carbonate (LeBlanc 
Process) — 175. Hydrolysis of Sodium Carbonate — 

176. Sodium Bicarbonate (C) — 177. Sodium Hydroxide — 

178. Electrolysis of Sodium Chloride (D) — 179. Borax (C) 

— 180. Borax Beads (C) — 181. Potassium — 182. Tests for 
Potassium (C*) — 183. Potassium Nitrate (C*) 

Calcium — Strontium — Barium.137 

184. Calcium Carbonate — 185. Tests for Calcium (C) — 

186. Testing for Calcium — 187. Calcium Oxide and Hydrox¬ 
ide (C*) — 188. Mortar —189. Cement — 190. Analysis of 
Cement (C) (Q) — 191. Hand Water (C*) — 192. Plaster of 





CONTENTS 


Vll 


Paris—193. Tests for Strontium and Barium (C*) — 194. 
Red Fire and Green Fire (D) 

Iron. 

195. Properties — 196. Slag — 197. Ferrous Compounds 
(C*) — 198. Ferric Compounds (C*) — 199. Reduction and 
Oxidation of Iron Compounds (C*) — 200. Hydrolysis of 
Ferric Chloride (C) — 201. Testing for Iron 

Aluminium. 

202. Properties —• 203. Aluminium Hydroxide (C) — 204. Clari¬ 
fication of Water— S 205. Thermit (D) — 206. Tests for Alu¬ 
minium (C*) — 207. Alum—208. Mordants—209. Hydrolysis 
of Aluminium Chloride (C) 

Copper . 

210. Properties — 211. Tests (C)—■ 212. Copper Sulphate 

— 213. Copper Alloys—-214. Displacement (Copper) (C*) 

Magnesium — Zinc — Mercury. 

215. Magnesium and Zinc—216. Tests for Magnesium (C) 

— 217. Testing for Magnesium—218. Tests for Zinc (C) — 
219. Zinc Hydroxide—220. Mercury —- 221. Mercurous and 
Mercuric Compounds (C) — 222. Displacement (Magnesium, 
Zinc, and Mercury) (C*) 

Tin — Lead. 

223. Tin and Lead — 224. Test for Tin (C) — 225. Tests 
for Lead (C) — 226. White Lead — 227. Displacement (Tin and 
Lead) (C*) — 228. Testing for Lead — 229. Qualitative Analy¬ 
sis (Lead, Silver, and Mercury) (C*) 

Silver — Gold. 

230. Tests for Silver (C) — 231. Displacement of Metals 
(Silver) (C*) — 232. Cleaning Silver—233. Silver Salts — 
234. Photography—235. Gold. 

Chromium — Manganese. 

236. Tests for Chromium (C) — 237. Potassium Chromate and 
Dichromate (C) — 238. Tests for Manganese (C) 

Appendix . 

Pressure of Water Vapor — Laboratory Equipment 

Index .... . 


PAGE 


142 


144 


147 


I48 


151 


153 


155 


158 

165 








Frontispiece 

Fig. I. — Apparatus frequently used in the laboratory 


















































































EXPERIMENTS 
IN PRACTICAL CHEMISTRY 

INTRODUCTION 


1 . General directions for the pupil. — The apparatus you will use 
frequently is shown on the opposite page. The pieces are lettered 
as follows: — 

A — Thistle tube. B — Test tube holder. C — Glass plate. D — 
Pinch clamp. E — Glass tube. F — Crucible block. G — Porcelain 
crucible (covered). H — Triangle. I — Forceps. J — Blowpipe tube. 
K — Test tube brush. L — Blowpipe. M — Right-angle bend. N — 
Glass rod. O — Porcelain evaporating dish. P — Glass plug. Q — Mor¬ 
tar and pestle. R — Rubber stopper (2-hole). S — Bottle. T —De¬ 
flagrating spoon. U — Rubber stopper (i-hole). V — Erlenmeyer flask. 
W — Iron clamp. X — Wire gauze. Y — Iron ring. Z —• Iron stand. 
AA —'Funnel. BB — Test tube (small). CC — Test tube (large). 
DD — Graduated cylinder. EE — Beaker. FF — Test tube rack 
(shown in part). 

Use Fig. I in preparing a list of the apparatus in your desk. 
When your set of apparatus agrees with the list, hand the com¬ 
pleted list to the Teacher. 

Some general apparatus will be found in the laboratory and special 
apparatus will be supplied as needed. Use this apparatus as directed. 

Besides the apparatus in your desk, you will need a rubber apron 
and a pair of sleeves, or something similar, to protect your clothes. 

You will need a laboratory notebook. Write your name and 
the number of your desk on the notebook. In this book you should 
keep a neat and accurate account of a-11 the experiments you perform. 
The Teacher will give special directions for writing the notes, handing 
in the book, and correcting errors. In general, your record of each 
experiment should include: — 

(1) The number and title of the experiment and the date. 

(2) An account of the experiment — brief, but full enough to 
permit a correct repetition of the experiment or its essential parts. 


2 EXPERIMENTS IN PRACTICAL CHEMISTRY 


(3) Answers to all questions — not merely yes or no, but an answer 
involving the question. 

(4) The numbers and letters which correspond to those in the 
directions, e.g. 1, I, (1), a, etc. 

(5) All numerical data, e.g. weights and volumes, in the form given 
in the directions. 

(6) A simple sketch of the apparatus (if time permits). 

(7) A table of contents. 

To do experiments successfully, you must meet certain require¬ 
ments. Before the laboratory period find out what experiment is to 
be done, read the directions carefully, and plan the work as well as 
you can. When you enter the laboratory, open your desk at once, 
or have it opened, take out the necessary apparatus, and begin to 
work without delay. When you are doing an experiment in the 
laboratory, follow the directions carefully, especially about quantities 
of chemicals, heating, and weighing; work and think independently. 
If you need assistance, ask the Teacher, not your neighbor. Your 
work will be more profitable if you follow these suggestions : — 

(a) Learn as soon as possible the name of each piece of apparatus, 
and how to use it. 

( b ) Learn how to perform skillfully the operations so frequently done 
in the laboratory, e.g. heating, filtering, weighing (see §§ 2, 4 ,8 below). 

(c) Learn how to set up apparatus, inspect it, and correct defects. 

(1 d ) Learn how to do arithmetical 

work quickly and accurately, and to 
check results. 

Before you leave the laboratory, be 
sure your apparatus is clean and put 
away, the water and the gas are turned 
off, and your desk is in just as good 
order as you would like to find it. 

2 . How to use the Bunsen burner. 
— The Bunsen burner (Fig. II) is 
used as a source of heat. It is attached to a rubber tube {A), 
which is connected with the gas supply. To light the burner, turn 
on the gas and hold a lighted match a short distance above the top 
of the burner tube ( B ). The flame should be a faint blue. If it is 
yellow, turn the ring at the bottom of the burner until the flame is blue. 



Fig. II. — Bunsen burner 











INTRODUCTION 


3 


A suitable height for most experiments is about io cm. (or 4 in.). 
Adjust the gas pressure until the flame is about this height. The hot¬ 
test part of the flame is near the top. 

In heating with the Bunsen burner follow these directions: — 

a. Light the burner before a piece of apparatus is held over it or be¬ 
fore it is placed beneath a wire gauze which supports a dish or a flask. 

b. Test tubes — used frequently — should be dry on the outside. 
If the test tube contains a solid, 
heat gradually by moving the tube 
in and out of the flame. If the test 
tube contains a liquid, only the part 
containing the liquid should be put 
in (or above) the flame. When 
the liquid begins to boil, the test FlG - IIL Cutting a glass tube 
tube should be removed from the flame for an instant or held over it. 
As a rule a test tube holder should be used (Fig. 3). 

c. Do not heat empty glass apparatus, e.g. beakers. In heating 
a beaker containing a liquid, do not use the free flame, but place the 
vessel on a wire gauze which stands on an iron ring. Porcelain 
dishes should also be placed on a gauze. Porcelain crucibles may 
be heated with a free flame. All porcelain apparatus should be 
heated and cooled gradually. 

3 . Cutting, bending, and drawing glass tubing. — a. Cutting. — 

Determine the length needed, lay 
\\ the tube on the desk, and with 

/ forward strokes of a triangular file 

/ ma ke a short, deep scratch where 

the tube is to be cut. Grasp the 
N/ 7 tube in both hands, and hold the 
thumbs together opposite the 
' scratch; now push gently with the 

- - thumbs, pull at the same time 

^= 32 ^ with the hands, and the tube will 

Fig. IV. ■ —• Fire polishing a glass break at the desired point (Fig. 

tube HI). The sharp ends should be 

smoothed by rotating them slowly in the Bunsen flame until a yellow 
color is distinctly seen or until the end becomes red hot; this operation 
is called fire polishing (Fig. IV). 









4 EXPERIMENTS IN PRACTICAL CHEMISTRY 



Fig. V. — A wing- 
top burner 


b. Bending.— Glass tubes can be bent in an ordinary illuminating 
gas flame, but the Bunsen flame is usually flattened by a wing-top 
(Fig. V). Attach the wing-top to the top of the 
burner tube before lighting the gqs. The flattened 
Bunsen flame should be slightly yellow and about 
7 centimeters (2.5 inches) wide for ordinary bends. 
A right-angle bend is easily made. Determine the 
part where the tube is to be bent. Grasp the 
tube in both hands, and hold it so that this part is directly over the 
flame (Fig. VI). Slowly 
rotate it between the 
thumbs and forefingers, 
and gradually lower it 
into the flame. Con¬ 
tinue to rotate it until 
the glass feels soft and 
ready to bend. Then 
remove it from the 
flame, and slowly bend FlG - VI - ~ Bending a tube into a right angle - 

it into a right angle ^ rst step 

(Fig. VII). Use a block of wood to assist the eye in making an 




Fig. VII. — Bending a tube into a 
right angle — second step 


Fig. VIII. — Bending a tube into 
an oblique angle — first step 


coated with soot, and then allowing it to cool slowly. Tubes 
can be bent into an oblique angle by heating them through 
about twice the space required for a right angle (Figs. 
VIII, IX); a very slight bend can be made by holding the 




























INTRODUCTION 


5 



tube across the flame, heating a short space, and then bending 
slightly. 

c. Drawing. — Glass tubes can be drawn into two pointed tubes 
thus: Heat the tube as in b through about 2.5 centimeters (1 inch) 
of its length, remove it from the 
flame and slowly pull it apart a 
short distance; let it cool for a 
few seconds, and then pull it 
quickly to the desired length. 

Stirring rods can be made from 
glass rod in the same way. 

4. Filtering. — A solid may be 
separated from a liquid by filter- Fig. IX. — Bending a tube into an 
ing. A circular piece of filter oblique angle - second step 
paper is folded to fit a glass funnel, and when the mixture is poured 
upon this paper the solid — called the residue or precipitate — is 

retained, while 
the liquid — 
called the fil¬ 
trate — passes 
through and may 
be caught in a 
test tube or any 
other vessel. 

The filter paper is prepared for the funnel by folding the circular 
piece A (Fig. X) into the shapes B and C. The folded paper is then 
opened so that three 
thicknesses are on one 
side and one on the 
other. To filter, the 
cone - shaped paper 
(from C) is placed in 
the funnel ( D) and 
moistened with water, 
so it will stick to the 
funnel. The liquid Fig. XI. - Funnel supported for filtering 

to be filtered may be poured directly from the vessel upon the 
paper or down a glass rod which touches the edge of the 



Fig. X. — Preparing a filter paper 




























6 EXPERIMENTS IN PRACTICAL CHEMISTRY 


vessel (6 a); the lower end of the rod should nearly touch the 
paper inside the funnel. The funnel can be supported as shown in 
Fig. XI. 

5 . Constructing and arranging apparatus. — The various parts 
of the apparatus should be assembled and put together as completely 
as possible before starting the experiment. The parts that are to 
fit each other should be connected so that all joints are gas-tight. 
In long experiments or those involving weighing the apparatus should 
be inspected by the Teacher. 

a. To insert a glass tube into a rubber tube. — Cut one end of the 
rubber tube at an angle, moisten the smoothed end of the glass tube 
with water, place the end of the glass tube in the angular-shaped 
cavity so that both tubes are at about a right angle, grasp the end 
of the rubber tube firmly and slip it slowly up and over the end of 
the glass tube. 

b. To push a glass tube through a hole in a stopper. — Wet one 
end of the tube with water and grasp it firmly near this end; hold 

the stopper between the thumb and fore¬ 
finger of the other hand, and work the tube 
through the hole by a gradual rotary motion. 
Never point the tube toward the palm of 
the hand that holds the stopper. Never 
grasp a bent tube at the bend when inserting 
it into a stopper — it may break and cut the 
hand severely. 

c. To bore a. hole in a cork. — Select a 
Fig. XII. —■ Cork borer cork free from cracks or channels and use a 
in a cork borer which is one size smaller than the de¬ 

sired hole. Hold the cork between the thumb and forefinger, press the 
larger end against a firm board, and slowly push the borer (previously 
moistened with water or soap solution) by a rojtary movement through 
the cork, taking care to bore perpendicularly to the cork (Fig. XII). 
If the hole is too small, enlarge it with a round file. Push the small 
cylinder of cork finally out of the borer with the handle. 

d. To make a test wire. — (i) Platinum. Rotate one end of a 
piece of glass rod, about io centimeters (4 inches) long, in the flame 
until it softens. At the same time grasp a piece of platinum wire 
about 7 centimeters (3 inches) long firmly in the forceps about 1 









INTRODUCTION 


7 


centimeter (0.5 inch) from the end, and hold it in the flame. When 
the rod is soft enough, gently push the hot wire into the rod. 
<0-^- ) 


¥> / / / 


5 


Fig. XIII. — Test wires — platinum (upper), nichrome (lower) 


(2) Nichrome. Wind a piece of nichrome wire around a match stick. 
The completed wires are shown in Fig. XIII. 

6 . Pouring liquids and transferring solids. — a. Liquids can be 
poured from a test tube or 
dish without spilling by 
moistening a glass rod 
with the liquid, holding 
the rod against the edge 
of the vessel, and then 
pouring the liquid slowly 
down the rod (Fig. XIV). 

b. Liquids should be 
poured from a bottle by 
holding the bottle as 

shown in Fig. XV. Note „ „ . r ., , , 

1 0 1 1 Fig. XIV. — Pouring a liquid down a rod 

that the stopper and bottle 

are held in the same hand. The stopper is first removed by hold¬ 




ing the palm of the hand upward and grasping the stopper between 
the fingers before the bottle is lifted (Fig. XVI). All stoppers 

























8 EXPERIMENTS IN PRACTICAL CHEMISTRY 


should be removed this way when possible, and not laid down on 
the desk. The drop on the lip of the bottle should be touched 
with the stopper before the latter is put into the bottle. 

c. Solids should never be 



poured directly from a large 
bottle into a test tube or 
dish. Use a spoon, spatula, 
or piece of smooth paper; 
or rotate the bottle slowly so 
that the solid will roll out 
in small quantities. If the 


Fig. XVII. Putting a solid into a tube so tid j s dirty ( e.g . charcoal ) f 
first step catch the solid on a nar¬ 


row strip of paper creased lengthwise, and introduce the solid from 
the paper into the test tube as shown in Figs. XVII, XVIII. 

7. Collecting gases. — Gases 
are usually collected over water 
in a pneumatic trough; one form 
is shown in outline in Fig. XIX 
(right). The bottle (or tube) to 
be filled with gas is first filled 
with water, covered with a piece 
of filter paper, inverted (Fig. XIX 
— left), and placed mouth down¬ 
ward on the support of the 
trough, which is previously filled 




Fig. XVIII. — Putting a solid into 
a tube — second step 


with water just above the support 
(Fig. XIX). The paper is then 
removed. Glass plates instead of 
filter paper may be used to cover 


!ig. XIX. Pneumatic trough in the bottle. The gas escapes from 

of^water (left ^'*'* the delive ^ tube > bubbks 

through the water into the vessel, 

and forces the water out of the vessel. Gases not very soluble in 
water (e.g. oxygen and hydrogen) are collected in this way. 



















INTRODUCTION 


9 



Fig. XX. 


Scales 


Some heavy gases, e.g. hydrochloric acid, chlorine, and sulphur 
dioxide, are collected by allowing the gas to flow downward into an 
empty bottle, i.e. by downward dis¬ 
placement (Fig. 41). Ammonia 
and other light gases are collected 
by allowing the gas to flow upward 
into a bottle, i.e. by upward dis¬ 
placement (Fig. 48). 

8 . Weighing. — Weighing may 
be approximate or accurate. Ap¬ 
proximate weighings are made on the scales (Fig. XX) and accurate 

weighings on the horn pan balance 
(Fig. XXI) or on the chemical 
balance (Fig. XXII). The Met¬ 
ric System of Weights is used 
and should be studied before weigh¬ 
ing is attempted. (See Appen¬ 
dix, § 1.) Note these general 
directions: — 

(1) Before weighing, see that 
the scales and balances are clean 
and properly adjusted. If out of 
order, do not adjust them your- 



Fig. XXI. — Horn pan balance 
hanging in a box (open in front 
and closed in back) to protect the 
balance from air currents 

self, but report to the Teacher. 

(2) Put objects on the left 
side and weights on the right. 
Heavy objects and weights 
should be put near the center of 
the pan. 

(3) Substances should not be 






i 


/ 

—at —a 



-f=Sr 


Fig. XXII. — Chemical balance in a 
glass case (front partly raised) 


placed directly on the platform or pan, except pieces of certain 
metals, e.g. zinc or aluminium, or porcelain and glass objects. 




























































io EXPERIMENTS IN PRACTICAL CHEMISTRY 


In weighing on the scales, put a piece of paper of about equal 
size on each platform; the paper on the left should be creased. Take 
the substance from the bottle with a clean spoon or spatula, or pour 
it out by rotating the bottle as described in 6 c above; if too much is 
taken out, do not put it back into the bottle, but throw it into the 
waste jar or a special bottle. Approximate weighings are made on 
the scales, e.g. the quantities of chemicals usually needed in or¬ 
dinary experiments. Objects and quantities weighing over ioo gm. 
should be weighed on the scales. 

In weighing on the horn pan or the chemical balance, if the sub¬ 
stance itself should not be placed directly on the pan, weigh a small 
watch crystal or crucible and then weigh the substance in this vessel. 
Sometimes a piece of apparatus is hung from the balance hook. Ac¬ 
curate weighings are made on the balance, e.g. the exact quantities 
needed in quantitative experiments. Record the total weight at 
once in the proper place in the Record in the laboratory notebook — 
not on a scrap of paper. Enter the weight as grams and a decimal 
fraction, e.g. 5.29 grams, not 5 grams, 2 decigrams, and 9 centigrams. 
Record all weighings — temporary and final — in the notebook. 

The process of weighing is as follows: — 

A. Scales. — Put the object, or the paper containing the proper 
substance, on the left side; on the right side put one or more weights 
which are judged to be the approximate weight. Now add or re¬ 
move (substance or) weights until the pointer swings the same num¬ 
ber of spaces each side of the middle division. Weighings of small 
quantities, e.g. 5 grams or less, are usually made by sliding a rider 
along a graduated beam on the front of the scales. 

B. Chemical balance. — Release the beam by turning the screw 
or lever. The pointer should swing the same (or very nearly the 
same) number of spaces each side of the central line. If it does not, 
consult the Teacher. If it does, proceed with the weighing. Put 
the* object {e.g. crucible, dish, tube, or special substance) on the left 
pan and the weight judged to be equal on the right pan. Release 
the beam carefully by turning the screw or lever, and note the move¬ 
ment of the pointer. If the added weight is correct, the pointer will 
swing the same (or very nearly the same) number of spaces each side 
of the central line on the scale. If incorrect (as it usually is), slowly 
turn back the screw or lever and bring the balance to rest. Add or 


INTRODUCTION 


ii 


remove the weight which is next heavier or lighter — as needed — 
and release again. If not correct, bring the balance to rest, and 
change the weights accordingly, taking care to add or remove the 
weights in order ( i.e. next heavier or lighter). Continue to change 
the weights, bringing the balance to rest each time, until the correct 
weight is obtained, i.e. when the pointer swings the same number 
of spaces each side of the central line as it did at the beginning. As 
soon as the substance or object is weighed, note the weights on the 
pan and record their sum at once in the notebook, then compare the 
weights with those missing from the box; if correct, so indicate in 
the notebook, and finally check the total weight by adding the weights 
as they are returned to the box. 

The following rules should be rigidly observed: — 

a. Always bring the balance to rest before changing the weights, 
the object, or the substance. 

b. If on releasing, the beam does not swing, arrest and release 
again, or fan one pan very gently. 

c. Handle all weights with the forceps — not the fingers. 

C. Horn pan balance. — The horn pan balance must be counter¬ 
poised before each weighing. This is readily done. Clean the pans 
with soft paper or cheesecloth. Allow them to swing freely and 
note which side is lighter by estimating the distances to right and 
left. Add bits of wire or compact wads of paper to the proper pan 
until the balance is counterpoised, i.e. until the pointer swings equal 
distances to the right and left. Proceed with the weighing as in B 
(noting that there is no releasing screw). 

9. Measuring. — Liquids are measured accurately in graduated 
cylinders and burettes (Figs. I, DD, 46). The lowest point of the 
curved surface of the liquid, called the meniscus, is its correct height 
(Fig. 47). 

Time can be saved by learning and remembering that the average 
ordinary test tube (15 X 1.8 centimeters or 6 X } inch) holds about 
30 cc. (cubic centimeters), while the large test tube (20 X 2.8 cen¬ 
timeters or 8 X 1 inch) holds about 75 cc. (cubic centimeters). 

10. Smelling and tasting. — Unfamiliar substances should never 
be smelled or tasted except according to directions, and even then 
with the utmost caution. Never inhale a gas vigorously, but waft it 
gently with the hand toward the nose. Never ask another pupil to 


12 EXPERIMENTS IN PRACTICAL CHEMISTRY 


inhale a gas. Taste acids, bases, and salts by touching a minute 
portion of the dilute solution to the tip of the tongue, and as soon 
as the sensation is detected, reject the solution at once — never 
swallow it. 

11 . Accidents. — Cuts should be washed in clean cold water and 
then covered with collodion or court plaster if slight, or bandaged 
if severe. 

Burns should be covered with a paste made by mixing sodium 
bicarbonate (baking soda) and carron oil (an emulsion of lime water 
and oil) and then bandaged. 

Acids and alkalies if spilled on the hands or spattered on the face 
should be washed off at once with water; if a burn is produced, this 
may be treated as described above. 

Fires may be extinguished by sand or by carbon tetrachloride. 
If the clothing catches fire, a damp towel or asbestos blanket should 
be used. 

An emergency box or cabinet containing “ first aid ” articles 
should be kept in a convenient place. For contents, see Appendix, § 6, 
List F. 


EXPERIMENTS 


CHEMICAL CHANGE — COMPOUNDS — ELEMENTS 

(Practical Chemistry, pp. i-io, §§ 1-14) 

Experiment 1 — Chemical Change 

Materials. — Candle, lime water. 

Apparatus. — Block of wood, bottle. 

Light a candle and stick it to a block of wood with a drop of melted 
candle wax. 

a. Hold a cold, dry bottle over the 
lighted candle (Fig. 1). Remove the bottle 
in a moment and examine the inside. 

Describe what you see. What is the sub¬ 
stance ? 

b. Pour some clear lime water into the 
bottle, and shake. Describe the change. 

What gas caused the change? 

Answer : 1. What are the two products of a 
burning candle ? 

2. Does the candle really “burn away”? Fig. i. — Studying a 

3. What does this experiment illustrate? chemica^ change 

Experiment 2 — Properties and Chemical Change 

Materials. — Sulphur, copper wire, concentrated nitric acid, magnesium 
ribbon. 

Apparatus. — - Test tubes, block of wood, forceps, Bunsen burner. 

a. Examine a piece of sulphur. Note and record its properties, 
e.g. color, odor, physical state. Put a small piece on a block of wood 
and light the sulphur by directing the flame upon it. Observe the 
color and size of the flame of the burning sulphur. Note (very 
cautiously) the odor of the gas by brushing a little gently toward the 
nose. 

Compare the properties (e.g. color, odor) of the gas with those of the 
sulphur. 



13 







14 EXPERIMENTS IN PRACTICAL CHEMISTRY 


What characteristic of chemical change does this experiment 
illustrate ? 

Do not let the sulphur burn longer than necessary. Extinguish 
it with a little sand, or by pressing it with a piece of stiff paper. 

b. Examine a piece of clean copper wire. Note and record its 
properties, especially color, appearance ( e.g . luster), and flexibility. 

Grasp one end of the wire with the 
forceps, and hold the other end in 
the hottest part of the Bunsen flame 
until the copper melts and undergoes 
a definite change (Fig. 2). Remove, 
and examine the product. Compare 
it with unheated copper. Is the 
product a different substance from the 
copper 



Fig. 2. — Heating copper wire 
in a Bunsen flame 


? Why? 

c. Roll a piece of copper wire into 
a ball, drop it into a test tube one 
fourth full of concentrated nitric acid, and warm gently. What is 
the evidence of chemical change? 

d. Examine a piece of magnesium ribbon. Note and record its 
properties, as in a. Grasp one end firmly with the forceps, hold the 
other end in the flame for an instant, and then remove it. Observe 
the result. Examine the product. How does it differ from magne¬ 
sium? 


Answer: 1. What is a conspicuous property of sulphur? Of copper? Of 
magnesium ? 

2. How does this experiment illustrate chemical change? 

3. What characteristic of chemical change does this experiment illus¬ 
trate? 


Experiment 3 — Mixture and Compound 

Materials. — Powdered sulphur, powdered iron (or clean, fine iron filings), 
dilute hydrochloric acid, carbon disulphide. 

Apparatus. — Scales, magnet, lens, test tubes and holder, Bunsen burner, 
mortar and pestle. 

Weigh about 4 gm. of powdered sulphur on a piece of paper on the 
scales (see Introduction §8A). Weigh about 7 gm. of powdered 
iron (or clean, fine iron filings) on another paper. 

a. Note and record their conspicuous properties. Try the effect 
of a magnet on each by moving it along the under side on the paper. 
Record the result. 






CHEMICAL CHANGE — COMPOUNDS 


15 

Put a pinch of each in separate test tubes, add a little dilute hydro¬ 
chloric acid, and warm gently. Note and record the result in each 
case, especially the odor of the gas from the tube containing the iron. 

Put a pinch of each in separate test tubes, add about 5 cc. of carbon 
disulphide, and shake well. (Caution. Carbon disulphide catches 
fire readily. Do not use carbon disulphide near a flame.) Note 
and record the result. 

Mix the sulphur and iron thoroughly by grinding them together 
in a mortar. Divide the mixture into two equal portions. Use one 
in b, and the other in c. 

b. Examine the mixture from a with a lens. Can you detect 
sulphur and iron? Try the effect of a magnet on some of the mixture, 
and state the result. 

Divide this portion into two parts. Put one part in a test tube, 
and add dilute hydrochloric acid. Warm the acid mixture gently 
until there is evidence of action, note the odor and compare with the 
odor from the iron and acid in a. 

Put the other part in a test tube, 
add 5 cc. of carbon disulphide, 
shake well, let it settle, pour the 
liquid into a dish, and stand the dish 
in the hood. When the carbon di¬ 
sulphide has evaporated, examine 
the solid product. What is it? 

c. Put the other half of the mix¬ 
ture from a in a test tube, attach 
the holder, and heat (Fig. 3). 

When the mass begins to glow, take 
the test tube out of the flame. Heat 
again intensely for a few minutes. Let the tube cool, hold it over 
the mortar, break off the lower end with the pestle. Remove the 
glass, grind the product, and use it in d. 

d. Examine the powder from c with a lens. Is iron or sulphur 
detected? Note and record the effect of a magnet. 

Put a pinch in a test tube, add a little hydrochloric acid, note 
the odor of the gas, and pour the contents immediately into a waste 
jar in the hood. Compare the odor of the gas with similar tests 
( e.g . in a). Is there evidence of iron? Of a new substance? 

Put a pinch in another test tube, add 5 cc. of carbon disulphide, 
and shake well. As soon as the solid has settled, pour the liquid 
into a dish, stand the dish in the hood, and let the liquid evaporate. 
Is any sulphur left in the dish ? 








16 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Answer: i. What are some characteristics of a mixture? Of a com¬ 
pound ? 

2. Is the product in c a mixture or a compound? Why? 

3. If the product in c had been weighed, how would its weight be related 
to the weight of the sulphur and iron ? 

4. How does this experiment illustrate the first characteristic of chemical 
change ? The second characteristic ? 

Experiment 4 — Compound and Elements 

Materials. — Oxide of mercury, joss stick (or small splint of wood). 
Apparatus. — Test tube clamped to iron stand (Fig. 4), Bunsen burner. 


J 


Put a little oxide of mercury (the same as mercuric oxide) on the 
end of a narrow piece of paper creased length¬ 
wise, and slip the powder into a test tube (Fig. 
5 ). The powder should nearly fill the round 
end of the test tube. Hold the test tube in a 
horizontal position, shake it to spread the 
powder into a thin layer, and then clamp the 
test tube as in Fig. 4 . 

a. Heat the whole test tube at first; then 
heat intensely the part that contains the sub¬ 
stance. After heating for several minutes insert 
a glowing joss stick well into the test tube. 
Observe and describe the change. The change 
is due to oxygen. If there is no change, heat 
intensely again and insert the glowing joss stick. 

b. Examine the deposit on the upper part of 
it? If you are in doubt, scrape out a little 

(Note. — Some unchanged 


Fig. 4. — Apparatus 
for decomposing 
oxide of mercury 


the tube. What is 
upon a piece of paper and examine it. 
oxide will probably be left; throw it in the waste jar.) 


Answer: 1. To what class of substances does mercuric oxide belong? 

2. To what class does the product from a belong? Fromb? 

3. Into what substances can mercuric oxide be decomposed? 


OXYGEN 


(Practical Chemistry, pp. 12-22, §§ 15-30) 

Experiment 5 — Preparation of Oxygen — Short Methods 

Materials. •— Lead dioxide, barium dioxide, potassium chlorate, sodium 
peroxide, hydrogen peroxide, dilute sulphuric acid, potassium perman¬ 
ganate solution, joss stick. 












OXYGEN 


n 


Apparatus. — Test tube clamped to an iron stand (as in Fig. 4), 
burner. 

(Note. — Hereafter the pieces of apparatus provided each pupil will 
not be included.) 

a. Put a little lead diox¬ 
ide into a test tube and 
proceed with the heating as 
in Exp. 4. If more con¬ 
venient, the substance may 
be heated as in Exp. 3 c 
(see Fig. 3). Test with a 
glowing joss stick. State 
the result. 

b. Proceed as in a, using 
barium dioxide. State the 
result. 

c. Proceed as in a, using potassium chlorate. State the result. 

d. Fill a test tube nearly full 
of water and stand it in the test 
tube rack. Obtain from the 
Teacher a little sodium peroxide 
on a creased paper, cautiously 
slip the sodium peroxide into the 
water, and put a glowing joss 
stick into the gas in the upper 
part of the test tube. State the 
result. 

e. Fill a test tube half full of 
fresh hydrogen peroxide, add 
half the volume of dilute sul¬ 
phuric acid, shake, and then 

Fig. s A. -Putting a powder into a nearl y fiU the test tube with 
test tube —second step potassium permanganate solu- 

tion. Immediately test the 
escaping gas with a glowing joss stick. State the result. 

Experiment 6 — Preparation and Properties of Oxygen— 
Long Method 

Materials. — 5 gm. of potassium chlorate, 5 gm. of manganese dioxide, 

joss stick, sulphur, piece of charcoal fastened to one end of a copper 

wire (30 cm. long), wad of iron thread (“steel wool”). 




Fig. 5. — Putting a powder into a test tube 
—• first step 






18 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Apparatus. — As in Fig. 6 . A is a large test tube (20 cm. or 8 in.) provided 
with a one-hole rubber stopper, to which is fitted a short glass tube B; 
the latter is connected by the rubber tube C with the delivery tube D. 
E is a pneumatic trough with a support for a collecting bottle. 

I. Preparation. — Weigh the potassium chlorate on the scales 
on a piece of paper creased lengthwise, and slip it into the test tube; 

Shake the test tube until 
the chemicals are thor¬ 
oughly mixed. Hold the 
test tube in a horizontal 
position and roll or shake 
it until the mixture is 
spread along about one 
half of the tube. Insert 
the stopper with its tubes, 
and clamp the test tube 
to the iron stand, as shown 
in Fig. 6, taking care 
not to crush the tube or 
disturb the contents. 
The end of the delivery tube D should rest on the bottom of the 
trough under the hole in the support. Be sure there are no leaks. 
Before proceeding, ask the Teacher to inspect the apparatus. 

Add water to the pneumatic trough E until the hole in the support 
is covered. Fill one bottle full of water, cover it with a piece of 
filter paper, invert it in the trough, remove the paper, and stand the 
inverted bottle upon, or near, the support (Fig. XIX). Fill three 
more bottles and have them ready to replace the one filled with gas. 

Heat the test tube gently with a small Bunsen flame about 10 cm. 
(4 in.) high. Move the flame slowly along the test tube, taking 
care not to heat the tube too long in one place nor too near the rubber 
stopper. As soon as the gas bubbles regularly through the water, 
slip the inverted bottle over the hole in the support. The gas will 
rise in the bottle and force out the water. If the gas comes off too 
rapidly, remove the flame for an instant; if too slowly, increase 
the heat; if not at all, examine the stopper and the rubber connecting 
tube for leaks, and adjust accordingly. 

When the first bottle is full of gas, remove it, cover it tightly with 
a piece of filter paper, and stand it (mouth upward) upon the desk. 
Invert another bottle in the trough, remove the paper, and slip the 
bottle over the hole. Fill it with oxygen. Fill all the bottles in the 


do the same with the manganese dioxide. 














OXYGEN 


19 


same way. When the last bottle of gas has been collected, im¬ 
mediately remove the end of the delivery tube D from the water. 
(Note. — After the test tube is cool, the contents can be removed 
with warm water.) Perform II at once. 

II. Properties. — a. Thrust a glowing joss stick into one bottle, 
and observe the result. Remove the joss stick, make it glow again, 
and repeat as many times as possible. How does the glowing joss 
stick change? Does oxygen burn? 

b. Put a small piece of sulphur in the deflagrating spoon, and 
heat it until the small, blue flame of burning sulphur is seen. Then 
lower the spoon into a bottle of oxygen. Notice any change in the 
flame. Very cautiously waft a little of the contents of the bottle 
toward the nose. Of what does the odor remind you? (As soon 
as the results are conclusive, remove the spoon and plunge it into the 
water in the trough to extinguish the burning sulphur. Cover the 
bottle with a piece of filter paper.) 

c. Heat the charcoal (fastened to the wire) long enough to produce 
a faint glow, then lower it into a bottle of oxygen. Observe the 
result. 

d. Twist one end of the copper wire (used in c) firmly around 
the wad of iron thread, heat the ends of a few strands for an instant, 
and quickly lower it into a bottle of oxygen. The iron should change 
conspicuously. Observe the result. 



Required Exercises. — 1. Write a brief 
account of Exp. 6 I in your notebook. 

2. Write a brief account of Exp. 6 II, answering all 
questions. 

3. State some physical properties of oxygen, e.g. 
color, solubility in water. 

4. Describe the chemical conduct of oxygen. 

5. (Optional.) Sketch the apparatus used to pre¬ 
pare oxygen. 

Experiment 7 — Oxidation of Copper 

Apparatus. — Evaporating dish, test tube fitted with 
a cork. 


Fig. 7. — Evaporat- p u t about 4 gm. of clean copper borings in 
ing dish on a gauze- an evaporating dish and stand the dish on a 
covered ring for gauze-covered ring attached to an iron stand 
oxidation of copper (jrjg 7). Heat the dish carefully but intensely 







20 EXPERIMENTS IN PRACTICAL CHEMISTRY 


about ten minutes. Then heat the contents of the dish directly 
with the free flame for about five minutes. Describe any marked 
change in the copper. 

When the dish is cool, transfer the contents to a test tube, cork 
tightly, and save for Exp. 23. (Note. — The dish can be cleaned 
by warming dilute nitric acid in it.) 

Answer: 1. What chemical compound was formed ? 

2. What elements combined? 

3. What general name is given to this kind of chemical change? 
What special name? 


Experiment 8 — Heating a Known Weight of a Metal in Air 

Material. — Zinc dust. 

Apparatus. — Crucible block (Fig. 8), covered crucible (Fig. 9). 


CD 


Cony the form of Record (see below) in your notebook. When 
you weigh, take the notebook to the bal¬ 
ance (or scales) and enter all weights in 
the proper place as soon as the weighing 
is made. Do this hereafter in all experi¬ 
ments which involve weighing. 

Clean and dry a porcelain crucible and 
cover. Place the covered crucible on the 



Fig. 8. 


- Block for carrying 
a crucible 


crucible block (Fig. 8), and carry it to the balance (or scales); always 
use this block in carrying the crucible to and from the balance (or 
scales). Weigh the covered crucible (see Introduction § 8 ). Enter 
the weight in the proper place in the Record. 


Record 


Wt. of crucible, cover, and zinc. gm. 

Wt. of crucible and cover. .gm. 

Wt. of zinc . gm. 

Wt. of crucible, cover, and contents after heating .... gm. 

Wt. of crucible and cover.. . gm. 

Wt. of contents after heating. gm. 

Wt. of zinc. gm. 

Change in weight. gm. 


Crease a slip of paper lengthwise, pour about 3 gm. of zinc dust 
into the crease, slide the zinc dust into the crucible (Fig. 5), and 
weigh accurately (including the cover). Enter the weight. 














OXYGEN 


21 


^>0 


Place the covered crucible on the triangle supported by a ring 
on an iron stand (Fig. o). Heat gently with a low flame to avoid 
breaking the crucible. Gradually increase the 
heat until the flame is just above the bottom of 
the crucible. Lift the cover occasionally by 
grasping the ring firmly with the forceps. If the 
zinc glows and a smoke escapes, cover the 
crucible at once to prevent loss. Heat for 
about twenty minutes. 

Cool the crucible gradually by moving the 
flame slowly beneath it. As soon as the 
crucible is cool, weigh. Enter the weight, and 
complete the Record. 

Show the final weight to the Teacher before 
throwing away the contents of the crucible. 

(Note. — The crucible can be cleaned with 
dilute hydrochloric acid.) Fig. 9. Covered 

crucible supported 

Answer: 1. What is the name of the product? on a Wangle 

2. What is the result of heating a known weight of a metal in air? 

3. To what is the difference in weight due? 


Experiment 9 — Slow and Rapid Oxidation 

(Demonstration Experiment) 

Materials. — Powdered potassium nitrate, charcoal, phosphorus-tipped 
match, bottle of oxygen, iron thread, phosphorus (for c), magnesium 
(for d), bottle of oxygen (for d). 

Apparatus. — As in Fig. to, iron pan. 

a. Lay a piece of charcoal on an iron pan, heat it with a direct 
flame, and when hot, cautiously sprinkle powdered potassium nitrate 
upon the hot surface. Stand back as soon as the chemical action 
begins. Observe the action, especially its violence and rapidity, 
also the effect on the charcoal. 

b. Rub the head of a phosphorus-tipped match with the finger 
in a dark place, and observe and describe the result. 

c. Teacher’s Experiment. Put a small piece of phosphorus 
(Care!) in an evaporating dish nearly full of water, cut off a thin 
slice, return the rest of the phosphorus to the bottle, and place the 
slice on an iron pan or a brick. Stand back, and observe the result. 









22 EXPERIMENTS IN PRACTICAL CHEMISTRY 



d. Teacher’s Experiment. Grasp one end of a short piece of 
magnesium firmly with the forceps, hold the 
other end in the flame for an instant, then re¬ 
move it, and let the magnesium burn in the air. 
In a similar way light another piece and quickly 
thrust it into a bottle of oxygen. Compare the 
results. In which case was oxidation more 
rapid ? 

e. Fill a test tube half full of iron thread, 
add io cc. of water, and moisten the iron. 
Cover the open end, and invert the test tube 
in a dish nearly full of water. Slip a rubber band 
upon the test tube to mark the height of the 
water, and clamp the test tube to the iron 


Fig. io. — Appara- 


tus for showing stan( j so that the Q p en enc j touches the bottom 
s ow oxi ation (jrjg IO ) L e t the whole apparatus 

stand undisturbed for a day or two, taking care to keep the open 
end of the test tube covered with water. Observe and explain the 
final result. 


Experiment 10 — Air and Combustion 

Materials. — Wood, paper, candle. 

Apparatus. — Two blocks of wood, lamp chimney. 

a. Set fire to a small piece of wood, drop it while burning into 
a bottle of air, and cover the bottle with a block of wood. Observe 
and state the final result. 

b. Proceed as in a, using a piece of paper and another bottle. 
Observe and state the final result. 

c. Attach a short candle to a block of wood with melted candle 
wax. Stand a lamp chimney tightly over the lighted candle. How 
is the flame affected? 

d. Hold the chimney a short distance (i cm. or 0.5 in.) above 
the lighted candle. Does the candle continue to burn? Why? 
Keep the chimney in the same position and cover the top with a 
block of wood. What is the result? Why? 

Answer: 1. What is your conclusion from these experiments about the 
relation of air to combustion ? 

2. Apply 1 to oxygen. 

3. How could the conclusion in 2 be verified by a simple experiment in 
the laboratory? 












CARBON AND ITS OXIDES 


23 


CARBON AND ITS OXIDES 

(Practical Chemistry, pp. 25-37, §§ 31-47) 

Experiment 11 — Distribution of Carbon 

Materials. — Sand, wood, cotton, starch, sugar, candle. 

Apparatus. — As in Fig. 11; block of wood. 

a. Cover the bottom of the crucible ( A ) with sand. Put in a 
small piece of wood, a wad of cotton, and a lump of starch. Fill 
the crucible with dry sand, and slip it into the ring 
of an iron stand (Fig. 11). Heat intensely until 
the smoking ceases (about 20 minutes). While 
the crucible is heating, proceed with b, etc. When 
the crucible is cool, pour the contents upon a block 
of wood or an iron pan. Separate the lumps from 
the sand. Examine and compare them with the 
original substances. What is the residue? 

b. Heat a little sugar in a test tube until 
the smoking ceases. What is the most obvious 
solid product ? 

c. Close the holes at the bottom of a lighted 
burner, and hold a glass tube in the upper part of 
the flame long enough for a thin deposit to form. 

Examine it. What is it? State its source. 

d. Hold a glass tube in the flame of a candle 
which stands on a block of wood, and note the 
with c. What is the deposit? 

Experiment 12 — Combustion and Carbon Dioxide 

Materials. — Copper wire, charcoal, limewater, wood, paper, denatured 
alcohol, gasolene. 

Apparatus. — Bent tube as in Fig. 12 for h. 

a. Wind one end of a copper wire around a small lump of charcoal, 
hold it in the flame until the edges glow, and then lower it into a bottle. 
Let it remain for a minute or two, then remove. Fill the bottle one- 
fourth full of fresh limewater, cover with the hand, and shake. Ob¬ 
serve and state the result. 

b. Recall and record the result of adding limewater to a bottle 
which was held over a burning candle. (See Exp. 1.) 



Fig. 11. — Appara¬ 
tus to show the 
distribution of 
carbon 

result. Compare 









24 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


c. Burn wood (e.g. a match) and paper in separate bottles and 
test as in a. State each result. 

d. Put several drops of denatured alcohol in an 
evaporating dish, set it on fire, and hold a bottle 
over the flame. Test as in a. State the result. 

e. Proceed as in d, using gasolene instead of 
alcohol (Care!). State the result. 

f. Hold a bottle over a low Bunsen flame for a 
minute or so, and then test as in a. State the 
result. 

g. Optional. Draw smoke through limewater, 
and state the result. 

h. Exhale the breath through a glass tube into 
a bottle half full of limewater (Fig. 12). De¬ 
scribe the result. What gas does the breath 



Fig. 12.-Testing contain? 

the breath Answer: i. Is carbon dioxide a product of com- 

bastion in each case? 

2. What are two tests for carbon in a compound? 


Experiment 13 — Fermentation and Carbon Dioxide 

(Demonstration Experiment) 

Materials. — Karo or molasses, yeast cake, limewater, kerosene. 
Apparatus. — Bottles and bent tube as in Fig. 13. 

Put 20 cc. of karo or molasses in a 250 cc. bottle (A in Fig. 13), 
add 175 cc. of water, and mix well. 

Grind one-fourth of a fresh yeast cake 
to a paste with about 10 cc. of water, add 
it to the solution and shake well. Fill 
the bottle B half full of limewater and 
cover this solution with a little kerosene 
(to protect it from the air). Connect as 
in Fig. 13 and let the apparatus remain 
a day or more where the temperature is 
25 0 to 30° C. 

Examine the liquid in B at intervals. Fig I3 ._ Apparatus to show 
What is the evidence that carbon diox- the relation of fermenta- 
ide is a product of fermentation? tion and carbon dioxide 
























CARBON AND ITS OXIDES 


25 


Experiment 14 — Preparation and Properties of Carbon 
Dioxide 

Materials. — Calcium carbonate, dilute hydrochloric acid, candle fastened 
to a wire, joss stick, calcium hydroxide solution. 

Apparatus. —■ As in Fig. 14. A is a 250 cc. bottle provided with a two-hole 
stopper, through which passes the dropping tube B and the right- 
angle bend C; the tube D (15 cm. or 6 in.) is attached to the bent 
tube by the rubber tube E. 

The dropping tube is made as follows: Cut off the top of a thistle 
tube about 2.5 cm. (1 in.) below 
the juncture of the stem and 
cup, and heat the sharp ends 
a minute or two in the flame; 
when cool, slip a thick-walled 
rubber tube (5 cm. or 2 in. 
long) over one end of the stem, 
attach a pinch-clamp to the 
rubber tube, and connect the 
tube with the cup, taking care 
to have the ends of the glass 
tubes as close together as 
possible. If properly con¬ 
structed, the cup will remain Fig. 14. Apparatus for preparing car- 
upright when full of liquid. bon dioxide 

Note. — Instead of the apparatus shown in Fig. 14, one of the simpler 
forms shown in Fig. 15 may be used; in 
these the end of the thistle tube must be 
beneath the acid. 

I. Preparation. — Put about 20 gm. of 
calcium carbonate into the bottle, and 
arrange the apparatus as in Fig. 14. Fill 
the pneumatic trough with water, fill a 
bottle with water, cover with filter 
paper, invert, stand it on the support, 
and remove the paper (see Fig. XIX). 
Fill three other bottles and have them 
ready. Introduce enough dilute hydro¬ 
chloric acid through the dropping tube 
B to cover the calcium carbonate. Car¬ 
bon dioxide will be evolved at once. 



Fig. 15. — Optional forms of 
apparatus for preparing 
carbon dioxide 













































26 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Collect four bottles, cover tightly with filter paper, and stand aside till 
needed. Proceed at once with II. 

II. Properties. — a. Plunge a blazing joss stick several times 
into a bottle. Observe and state the result. 

b. Lower a short, lighted candle into a bottle of air, and quickly 
invert a bottle of carbon dioxide over it, holding the bottles mouth 
to mouth. Observe and state the final result. 

c. Pour a little calcium hydroxide solution into a bottle of carbon 
dioxide, cover with the hand, and shake vigorously. Describe 
and explain the result. 

d. Fill a bottle of carbon dioxide one-third full of water,' cover it 
tightly with the hand, and shake vigorously. Invert the bottle, still 
covered, in the pneumatic trough and remove the hand. Observe 
and state the result. 

Note. — As soon as d is performed wash the acid from the marble and 
save the solid for other experiments. 

Answer: i. Describe briefly the preparation of carbon dioxide. 

2. What do a and b show about the relation of carbon dioxide to com¬ 
bustion? 

3. What does b show about the relative weights of carbon dioxide and 
air? 

4. What does d show about the solubility of carbon dioxide ? 


Experiment 15 — Beverages and Carbon Dioxide 



Fig. 16. — A siphon 
of water charged 
with carbon dioxide 


(Demonstration Experiment) 

Materials. — Siphon of charged water, bottle of 
ginger ale (or similar beverage), calcium hydrox¬ 
ide solution, joss stick. 

Apparatus. — As in Fig. 16, bent tube fitted to a 
one-hole stopper, beaker (or bottle.) 

a. Draw off some charged water from a 
siphon (Fig. 16) into a beaker (or bottle), and 
let it stand a minute or two. Then show the 
presence of carbon dioxide in the beaker (or 
bottle). 

b. Remove the metal cap from a ginger ale 
bottle, pour off a little of the liquid, and insert 
the rubber stopper with its tubes and arrange 
the apparatus so that the outer end rests on 








CARBON AND ITS OXIDES 


27 


the bottom of an empty beaker (or bottle). Let the whole remain 
undisturbed a few minutes, and then 
show that the beaker (or bottle) 
contains carbon dioxide. 

c. Proceed as in ( b ) with the same 
bottle, but fill the beaker (or bottle) 
half full of calcium hydroxide solu¬ 
tion, and have the outer end of the 
tube dip beneath the surface of the 
solution (Fig. 17). If necessary, warm 
the bottle of ginger ale. 

Answer: 1. What is the evidence 
of carbon dioxide in these experiments ? 

2. What is the evidence that the car¬ 
bon dioxide was under pressure in the 
siphon and the bottle? In which was Fig. 17. —Testing the gas from 
the pressure greater? a charged beverage 

Experiment 16 — Plants and Carbon Dioxide 

(Demonstration Experiment) 

Materials. — Fresh green leaves, water saturated 
with carbon dioxide, joss stick. 

Proceed as in the author’s Practical Chemis¬ 
try , bottom of page 31. Use the apparatus 
shown in Fig. 18. 

Required Exercises. — 1. Describe this ex¬ 
periment. 

2. What is the evidence that green plants (a) 
absorb carbon dioxide and ( b ) give off oxygen ? 

Experiment 17 — Fire Extinguishers and 
Carbon Dioxide 

(Demonstration Experiment) 

Materials. — Dilute sulphuric acid, saturated 

^ „ sodium bicarbonate solution. 

Fig. 18. — Experiment 

to show the relation Apparatus. — Bottle with one-hole stopper and 
of carbon dioxide to tubes as in Fig. 20, fire extinguisher (the port- 
plants able type as in Fig. 19). 



































28 EXPERIMENTS IN PRACTICAL CHEMISTRY 


a. Add dilute sulphuric acid to a test tube half full of saturated 
sodium bicarbonate solution and show that the escaping gas is car¬ 
bon dioxide. 

b. Unscrew the top of a portable fire extinguisher 
(Fig. 19) and examine the parts, noting especially 
the opening of the escape tube, bottle of acid, stop¬ 
per, and collar. Remove a little of the solution, 
and test it as in a. Replace the cap, take the ex¬ 
tinguisher to the roof, yard, or street and show how 
to use it in extinguishing a small fire. 

c. Optional. Make a simple extinguisher like 
that shown in Fig. 20. The bottle and tubes are 
those used (as A-C-E-D ) in the apparatus shown in 
Fig. 14. The bottle is filled about two-thirds full 
with saturated sodium bicarbonate solution, the 
small tube (inside the bottle) contains dilute sul¬ 
phuric acid and a piece of lead to hold it down 
after it is lowered into the solution. Connect the 

Fi G . 19. — Port- tubes with the stopper and push the stopper well 
able fire extin- down into the neck of the bottle, 
guisher (cut Build a small fire in a dish or on some bricks, 
away to show Hold the end of the tube in one hand, with 
acid bottle) the 0 ther grasp the bottle by the neck, taking 
care to hold the stopper tightly 
with the fingers, invert the 
bottle, and direct the stream 
upon the fire. 

Answer: 1. Why are sulphuric 
acid and sodium bicarbonate used in 
a fire extinguisher? 

2. Why does the liquid flow out 
of a fire extinguisher with such 
force? 

3. Does a “chemical” fire engine 
differ essentially from a portable extinguisher? If so, how? 

Experiment 18 — Carbon Monoxide 

(Demonstration Experiment) 

Proceed as in Exp. 142, or postpone until carbon monoxide is studied. 



Fig. 20. — Simple modification of a 
fire extinguisher 























HYDROGEN 


29 


HYDROGEN 

(Practical Chemistry, pp. 39-48, §§ 48-57) 

Experiment 19 — Preparation of Hydrogen — Short Methods 

Materials. — Zinc, magnesium, aluminium, iron, dilute hydrochloric acid, 
dilute sulphuric acid, sodium hydroxide. 

a. Fill a test tube half full of dilute hydrochloric acid, stand it 
in the rack, and drop in a small piece of zinc. Test the escaping gas 
by holding a lighted match at the mouth of the test tube. (If the 
test is not decisive, add more zinc, warm gently, or wait until more 
gas accumulates in the test 
tube.) What gas is it? What 
was its source? 

Proceed in the same way 
with magnesium and iron (in 
the form of tacks or filings); 
use separate test tubes, and 
heat, if the action is slow. 

Observe the result in each 
case, and apply the questions 
asked about zinc. 

b. Proceed as in a, using 
dilute sulphuric acid. Observe 
the result in each case. Answer 
the questions asked in a. 

c. Roll two or three small, thin pieces of aluminium into a ball, 

drop it into a test tube, slip in a piece of sodium hydroxide about 2.5 

cm. (or 1 in.) long, and add a little water. Warm gently. Observe 

the result, and test as above. Answer the questions asked in a. 

Experiment 20 — Preparation and Properties of Hydrogen — 
Long Method 

Materials. — 10 gm. of granulated zinc, dilute sulphuric acid, copper 
sulphate solution, wax taper. 

Apparatus. — As in Fig. 21. See also Fig. 15 for optional forms. 

I. Preparation. — Slip the zinc into the bottle (or test tube) 
— Fig. 21. Insert the stopper with its tubes. Be sure there are 
no leaks. Fill the pneumatic trough with water as usual, and ad- 



Fig. 21. — Apparatus for preparing 
hydrogen 



















30 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


just the apparatus so that the end of the delivery tube rests on the 
bottom of the trough under the hole in the support. Fill the bot¬ 
tles with water, and cover each with filter paper; invert one in 
the trough, remove the paper, and stand the inverted bottle upon 
the support (see Fig. XIX). 

Put 2 or 3 cc. of copper sulphate solution in the cup, fill with dilute 
sulphuric acid, and let the acid mixture run into the bottle by pinch¬ 
ing the clamp ; if the acid does not flow freely down the tube into the 
bottle, loosen the stopper for an instant. (The copper sulphate has¬ 
tens the chemical change.) The gas will bubble through the water 
up into the bottle. 

Collect and remove four bottles of gas as in the Preparation of 
Oxygen (Exp. 6), taking care to cover each bottle tightly with a piece 
of wet filter paper. If the evolution of gas slackens or ceases, add 
a little more acid through the dropping tube. Perform II at once. 

II. Properties. — a. Uncover a bottle for an instant to let a little 
air in, and then hold a lighted match at the mouth of the bottle. Ob¬ 
serve the result. 

b. Remove the paper from another bottle and allow it to remain 
uncovered for three minutes — by the clock. Then show the pres¬ 
ence or absence of hydrogen by holding a lighted match at the mouth 
of the bottle. Observe the result. What property of hydrogen 
does this experiment show? 

c. Stand a covered bottle of hydrogen on the desk, place a bottle 
of air over it, remove the paper, and bring the mouths of the bottles 
together. Let them remain in this position for a minute or two, 
then remove the upper bottle and cover both with wet filter paper. 

Remove the paper from one bottle and hold a lighted match at 
the mouth. Observe the result. Do the same with the other bottle. 
What property of hydrogen does this experiment show? 

d. Invert a covered bottle of hydrogen, remove the paper, and 
quickly thrust a lighted taper up into the bottle. Withdraw the taper 
slowly. Then insert and withdraw it several times, and observe 
carefully (i) if the hydrogen burns, (2) if so, where, and (3) if the 
taper burns both inside and outside the bottle. Feel of the neck of 
the bottle; describe and explain. What properties of hydrogen 
are shown by this experiment? 

Note. — As soon as II is completed, wash the zinc several times, and 
save it for other experiments. 

Required Exercises. — 1. Write a brief account of Exp. 20 I. 

2. Write a brief account of Exp. 20 II, answering all questions. 


HYDROGEN 


31 


3. State the conspicuous physical properties of hydrogen. 

4. What is a test for hydrogen? 

5. Why was there an explosion in a? Why none in d? 

6. Does hydrogen support combustion? 

7. (Optional.) Sketch (from memory, if possible) the apparatus used 
to prepare hydrogen. 

Experiment 21 — Interaction of Water and Sodium 

(Demonstration Experiment) 

Materials. — Sodium, tea lead (or wire gauze). 

Apparatus. — Test tube clamped over dish as in Fig. 22. 

Caution. — Sodium is a dangerous substance. It should be handled 
cautiously and used strictly according to directions. Small frag¬ 
ments obtained for experiments should be pro¬ 
tected from water by a mortar or dish. If any 
sodium is left from an experiment, it must not 
be thrown into the refuse jar, but returned to 
the bottle. 

Fill an evaporating dish two-thirds full of 
water. Fill a test tube full of water, cover and 
invert it, and clamp it as shown in Fig. 22. 

Wrap a small piece of clean sodium loosely in a 
piece of dry tea lead about 5 cm. (2 in.) square, 
make two or three small holes in the tea lead, 
and slip it under the test tube. (Wire gauze 
may be used instead of tea lead.) A gas will Fig. 22. Appara- 
rise in the test tube. Proceed similarly with 
additional pieces of sodium and dry tea lead 
until the test tube is full of gas. Then unclamp 
it, keep it mouth downward, and hold a lighted 
match at the mouth. Observe the result imme¬ 
diately, especially at the mouth of the tube. What is the gas? 
What was its source ? 

Experiment 22 — Burning Hydrogen 

(Demonstration Experiment) 

Materials. — 20 gm. of granulated zinc, dilute sulphuric acid, copper sul¬ 
phate solution, platinum wire (optional), small bottle. 

Apparatus. — As in Fig. 23. The platinum tip is shown (about actual 
size) in Fig. 24. Directions for making the platinum tip may be found 


tus for collecting 
the gas liberated 
by the interaction 
of water and so¬ 
dium 













32 EXPERIMENTS IN PRACTICAL CHEMISTRY 


in the author’s Experimental Chemistry , page 340. If platinum is not 
available, a piece of capillary glass tubing about 5 cm. (2 in.) long 
may be used. 



Fig. 23. — Apparatus for burning hy¬ 
drogen 


Caution. — Perform this experiment with extreme care, since a 
mixture of hydrogen and air explodes violently if ignited. 

Put the zinc in the bottle 
(Fig. 23). Fill the U-tube 
two-thirds full of calcium chlo¬ 
ride, put a wad of cotton 
upon the solid, insert the 
stopper in each arm, and con¬ 
nect the U-tube with the gen¬ 
erator and the exit tube. Ex¬ 
amine all joints to be sure they 
are tight. Extinguish all 
flames in the vicinity, and 
proceed exactly according to 
directions. 

Introduce through the drop¬ 
ping tube about 25 cc. of dilute 
sulphuric acid containing 5 cc. of copper sulphate solution. Acid 
may be added slowly after the evolution of gas begins, but no air 
should be introduced. 

Let the gas bubble through the acid two minutes, then 
attach the rubber connector and the capillary glass tube 
(or the platinum tip) to the end of the exit tube, leaving 
a short space between the ends of the two glass tubes so 
the rubber tube may be compressed suddenly, if necessary. 

Let the gas run half a minute to drive air out of the tip 
(Fig. 24). 

Slip a small test tube over the tip, and when it is full of 
hydrogen gas remove the test tube (still inverted or 
closed with the thumb), take it a few feet away from the 
generator, and hold a lighted match at the mouth; if an 
explosion results, collect another test tube and test again, 
repeating until the gas lights with only a faint noise and . a lnum 
burns quietly at the mouth of the tube. Then light the p 
hydrogen at the tip, and observe at once the faint flame. 

a. Show that the flame is very hot by holding a match or platinum 
wire over it. 

b. Hold a small, dry bottle over the flame in such a position that 

























HYDROGEN 


33 


the tip of the flame is just inside the bottle. Note the deposit in¬ 
side the bottle. Remove the bottle, and extinguish the flame at 
once by pinching the rubber connector. Examine the inside of the 
bottle. What is the deposit? Explain its formation. 

Answer : i. What is the product of burning hydrogen ? 

2. How does this experiment illustrate oxidation? Combustion? 


Experiment 23 — Reduction of Copper Oxide by Hydrogen 

Materials. — Copper oxide, io gm. of granulated zinc, dilute sulphuric 
acid, copper sulphate solution. 

Apparatus. — As in Fig. 25. The parts lettered A, B, C, D, E constitute 
the hydrogen generator used in Exp. 20. F is a large test tube fitted 
with a two-hole stopper; the delivery tube E passes through one hole 
and extends nearly to the bottom of the test tube. The right-angle 
tube G passes just through the other hole; the tube G is lengthened 
by the rubber tube H. 


While the parts of the apparatus are being collected and arranged 
put the copper oxide prepared in Exp. 7 in an evaporating dish, stand 
the dish on a gauze- 
covered ring attached to 
an iron stand (Fig. 7), 
and heat gently. (If 
Exp. 7 was omitted, use 
5 gm. of copper oxide.) 

Slip the copper oxide 
into the dry test tube F 
(Fig. 25), hold the tube 
in a horizontal position 
and tap it gently to 
spread the solid into a 
thin layer. Connect this 
test tube with the rest of 
the apparatus, and clamp 
it into the proper posi¬ 
tion, taking care not to 



Fig. 2- 


— Apparatus for the reduction of 
copper oxide by hydrogen 


crush the tube. Put the zinc into the 


bottle A. 

Ask the Teacher to inspect the apparatus, and do not proceed un¬ 
til permission is given. After obtaining permission, put 2 cc. of cop¬ 
per sulphate solution into the cup, fill the cup nearly full with dilute 
sulphuric acid, pinch the clamp, and let about half the acid run into 


























34 EXPERIMENTS IN PRACTICAL CHEMISTRY 

the generator bottle. If the hydrogen does not bubble freely, let 
more acid run in, taking care to keep a little acid in the cup. Add 
enough acid to keep the gas flowing steadily through the apparatus 
for at least two minutes before lighting the Bunsen burner. 

Heat gently the lower part of the test tube where the copper oxide 
is located. Do not let the flame come near the rubber tube H. The 
gas must flow slowly through the apparatus during the heating; if 
it does not (as you can tell by the bubbles in the bottle or by smell¬ 
ing the gas at the end of the rubber exit tube), introduce more acid. 
If the test tube F should break, pinch the rubber tube D an instant 
to cut off the flow of hydrogen, and then extinguish the Bunsen burner 
flame. 

Continue to heat until a marked and permanent change is observed 
inside the test tube F. Then stop heating, and extinguish the Bunsen 
burner flame at once. Note the two products in the test tube (dis¬ 
regarding any unchanged copper oxide). What is each product? 

Required Exercises. — i. Describe briefly the whole experiment, 
and sketch the apparatus. 

2. What chemical compound was formed in F? 

3. How was the copper oxide changed? What special name is given to 
this kind of change? 

4. Recall Exp. 7 (Oxidation of Copper). In Exps. 7 and 23, what was 
oxidized, what was reduced, and what substances accomplished the oxida¬ 
tion and the reduction? 

5. Summarize in a few words how Exps. 7 and 23 illustrate oxidation and 
reduction. 


MEASUREMENT OF GASES 

(Practical Chemistry, pp. 50-57, §§ 58-66) 

Experiment 24 — Weight of a Liter of Oxygen 

Note. — This Experiment may be postponed until the pupil has acquired 

more experience in the laboratory. 

Object. — To find the weight of a certain volume of oxygen, reduce this 
volume to standard conditions, and calculate the weight of 1 liter of 
oxygen. (N ote. — See Introduction, § 8, for directions about weighing.) 

Materials. — Potassium chlorate, manganese dioxide, calcium chloride, 
glass wool or shredded asbestos. 

Apparatus. — As in Fig. 26. A is a test tube attached to the bent tube 
F by a rubber stopper. B is a large bottle (2500 cc.) to be filled with 


MEASUREMENT OF GASES 


35 


water; it is provided with a two-hole rubber stopper, through which 
pass F and C, the latter being connected with a rubber tube C' to which 
is attached the short glass tube G. A Hofmann screw is attached at 
the point E. Another bottle (2500 cc.) D serves to catch the water 
forced over from B through CC' by the oxygen generated in A . The 
hook 5 of aluminium wire permits A to be hung from the balance beam 
in weighing. Thermometer, barometer. 

Copy the form of Record, as given below, in the notebook. Enter 
all weights and volumes in the proper place as soon as the weighing 
and measuring are done. 

Fill the space 1 in A with a mixture of equal weights of powdered 
manganese dioxide and powdered potassium chlorate (Fig. 26). 
The mixture should 
be dried before use 
by heating it in an F 
oven to about no° 

C. Push glass wool, 
or shredded asbes¬ 
tos (previously ig¬ 
nited to a red heat), 
into the space 2 in 
A . Put small lumps 
of calcium chloride 
into 3 and glass 
wool into 4. Push 
the stopper well into 
the test tube. Wipe jr IG ^ — Apparatus for finding the weight of a 
A carefully with liter of oxygen 

soft paper. Weigh 

AF accurately on the balance and enter the weight in the proper 
place in the Record. Weigh the empty, dry, clean bottle D to a 
decigram on the scales, and record the weight. 

Fill B with water nearly to the neck. Fill CC' with water and 
tighten the Hofmann screw to prevent the water from running out. 
Insert F into the stopper of B. Push the stopper into the bottle, 
slowly at first, then hard; if water rises in F, loosen the screw at E 
slightly, remove A, and blow gently into F to force the water back 
into B. When properly adjusted, the water should be in B and CC' 
but not in F. Replace A, taking care not to crush the thin glass 
by pushing it too hard upon its stopper. Open the screw at E. If 
the apparatus is tight, little or no water will flow out. It should be 
adjusted until air tight. Leave the screw open. 





















36 EXPERIMENTS IN PRACTICAL CHEMISTRY 

Heat A gently with a low flame, keeping the flame back of the 
space 2 . The liberated oxygen will force the water from B into D. 
Heat A just hot enough to cause a gentle flow of water into D. When 
B is about half empty, stop heating. While A is cooling sufficiently 
to weigh, stand a thermometer in D ; also read the barometer. When 
A is cold, raise B until the water is at the same level in B and D, 
pinch C' tight and remove it from D. Read and remove the ther¬ 
mometer. 

Dry D on the outside, if necessary, and then weigh it on the scales; 
record the weight. The gain in weight (in grams) of D gives the 
volume of oxygen liberated (since i gm. of water = i cc.). 

Weigh AF on the balance; record the weight. Its loss in weight 
is the weight of the oxygen that passed into B. 


Record 

Weight of tube AF before heating.. . 

Weight of tube AF after heating.. . 

Weight of oxygen (W) . 

Weight of bottle D and water. 

Weight of bottle D empty. 

Weight of water . 

Volume of water. 

Observed volume of oxygen (F'). 

Temperature (t) . 

Pressure read on barometer (P'). 

Pressure caused by water vapor (a) . 

Corrected pressure. 

Corrected volume of dry oxygen (F). 

Corrected volume of dry oxygen expressed in liters (VI) 
Weight of i liter of oxygen. 


gm. 

.gm. 

gm. 

gm. 

. gm. 
gm. 
cc. 
cc. 
°C. 
mm. 
mm. 


cc. 

1 . 

gm. 


Correct the observed volume (F 7 ) of oxygen for temperature (t ), 
pressure (P'), and pressure of water vapor (<z). That is, reduce the 
observed volume to the volume (F) it would occupy, if it were at 
o° C., 760 mm., and in the dry state (i.e. free from water vapor). 
Water vapor exerts a pressure. Hence the pressure for which the 
observed volume (F') must be corrected is the observed pressure (P') 
minus the pressure due to the water vapor (a) in the gas (see § 74 in 
the author’s Practical Chemistry ). This complete correction is made 
by this formula: — 


273 


P' - a 


V = V' X 


273 + t 


X 


760 



















WATER — HYDROGEN PEROXIDE 


37 


The values for a at different temperatures are given in the Table in 
the Appendix. 

Since i liter contains 1000 cubic centimeters, then V -5- 1000 is 
the actual volume of liberated oxygen expressed in liters {VI). The 
weight of liberated oxygen (W) is found by subtracting the weight 
of HE after heating from its weight before heating. And finally the 
weight of i liter of oxygen in grams is found by dividing the weight 
of liberated oxygen by its volume, i.e. W -£■ VI. 


WATER — HYDROGEN PEROXIDE 

(Practical Chemistry, pp. 59-84, §§ 67-95) 

Experiment 25 — Water in Food and Other Substances 

a. Heat a small piece of meat in a dry test tube. Hold the open 
end of the test tube lower than the closed end, and take care not to 
burn the substance. What substance is liberated? 

b. Proceed as in a, using a dry test tube in each case and a small 
piece of the following: Potato, apple, cranberry, celery, bread, 
cracker. Observe and state the result in each case. 

c. Proceed as in b with wood, soft coal, fresh grass or leaves, hay, 
raisins or other kinds of dried fruit. Observe and state each result. 

d. How would you find the approximate per cent of water in bread, 
potato, or meat ? Before proceeding, submit the details to the 
Teacher. Compare the result with the per cent given in the author’s 
Practical Chemistry , § 377. 

Experiment 26 — Purification of Water 

Materials. — Water (100 cc.) rendered turbid with fine clay; cotton, 
sand, powdered charcoal, alum solution, ammonium hydroxide. For 
d bad smelling water, chlorine water. 

Apparatus. — Two funnels, test tube fitted with a cork (for d). 

a. Put a loose plug of cotton in the apex of a funnel, fill the funnel 
half full of sand, pour 25 cc. of the turbid water on the sand, and 
catch the filtrate in a test tube. (Meanwhile do b, etc.) Compare 
the filtrate with the sample. State the result. 

b. Proceed as in a, using fine wood charcoal instead of sand. Com¬ 
pare the filtrates from a and b with the sample. State the result. 

c. Fill a large test tube about four-fifths full of the turbid water. 
Add about 5 cc. of alum solution and mix well. Then add about 10 


38 EXPERIMENTS IN PRACTICAL CHEMISTRY 


cc. of ammonium hydroxide, and mix well again. Let the fix¬ 
ture stand undisturbed several minutes. Compare the upper liquid 
with the sample and with the filtrates from a and b. State the re¬ 
sult. 

d. Optional. — Add 2 cc. of chlorine water to a test tube nearly 
full of bad smelling water, cork, shake well, and then compare with 
the sample. State the result. 


Experiment 27 — Distillation of Water — Short Method 

Materials. — Copper sulphate and barium chloride solutions, ammo¬ 
nium hydroxide. 

Apparatus. — As in Fig. 27. A and B are large test tubes, and C is a 250 
cc. bottle. 

Put about 15 cc. of water in the test tube A , add 2 or 3 cc. of copper 
sulphate solution (to color the water), and 
slip in two short pieces of glass tubing (to 
prevent “bumping”)- Arrange the ap¬ 
paratus as in Fig. 27. B is empty and C 
should be about three-fourths full of cold 
water. 

Heat the water in the test tube A to 
boiling. The steam passes into the test 
tube B and is condensed by the cold water 
in the bottle C. Continue to heat until 
about 10 cc. has collected. Compare the 
color of the distillate in B with the copper 
sulphate solution. State the result. Test 
half of the distillate for a sulphate by add¬ 
ing barium chloride solution (see Exp. 28 d (2)). Test the rest for 
copper by adding ammonium hydroxide. If copper is present, the 
solution will become deep blue. State each result. 



Fig. 27. — Apparatus for 
distillation of water 


Experiment 28 — Preparation and Properties of Distilled 
Water 


Materials. — Water containing a little dirt, calcium chloride, and sodium 
sulphate; potassium permanganate, silver nitrate, barium chloride, 
and ammonium oxalate solutions. 

Apparatus. — Liebig condenser, etc., as in Fig. 28. 

I. Preparation. — For the Teacher. Fill the flask A half full of 
the water containing the three impurities mentioned above, add a 











WATER — HYDROGEN PEROXIDE 


39 


few short pieces of glass tubing to insure even boiling, and connect 
with the condenser at B as shown in Fig. 28. Attach the inlet (lower) 
tube C to the faucet, fill the condenser slowly, and regulate the cur¬ 
rent so that a small stream flows continuously from the outlet tube 
D into the sink or waste pipe. 

Heat the liquid in A gradually to boiling, and then regulate the 
heat so that the boiling is not too violent. Reject the first 5 or 10 cc. 



Fig. 28. — Liebig condenser arranged to distil water 


of the distillate; they may contain impurities. As the distillate 
collects in the clean receiver E, proceed with the tests as in II. 

II. Properties. — For the Class, a. Taste of the distilled water. 
Compare with faucet or well water. 

b. Test distilled water for dissolved gases by heating a little in 
a clean test tube. State the result. Compare with faucet water. 

c. While the distillate is collecting, test the impure water for or¬ 
ganic matter. Put 10 cc. of the impure water in a test tube, 
add a few drops of concentrated sulphuric acid, and enough 
potassium permanganate solution to color the mixture a light reddish 
purple. Mix well by stirring with a glass rod. Grasp the test tube 
with the test tube holder and heat gently until the liquid begins to 
boil, taking care to remove the test tube from the flame occasionally 
to prevent the liquid from spurting out. If organic matter is present, 
the color of the solution will be changed to brown. 

Test in the same way 10 cc. of the distilled water, taking care to 
use a very clean test tube. Compare the results. 

d. Test separate portions (about 10 cc.) of the impure water for 
different kinds of mineral matter. In a similar way test the dis¬ 
tilled water and compare the corresponding tests. 


















40 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


(1) Chlorides. — Add a few drops of silver nitrate solution. The 
white, curdy solid is silver chloride, which is formed by the chemical 
action between silver nitrate and the dissolved chloride. All soluble 
chlorides produce the same result. Does the distilled water con¬ 
tain chlorides? 

(2) Sulphates. — Add a few drops of barium chloride solution. 
The white, fine precipitate is barium sulphate, which is formed by 
the chemical action between barium chloride and the dissolved sul¬ 
phate; its formation is a test for any sulphate in solution. Does 
the distilled water contain sulphates? 

(3) Calcium (or lime) compounds. — Add a few drops of ammonium 
oxalate solution. The white precipitate is calcium oxalate. Its 
formation serves as a test for dissolved calcium compounds. Does 
the distilled water contain calcium compounds? 

Experiment 29 — Some Physical Properties of Water 

Materials. — Ice, copper wire. 

Apparatus. — Test tube with one-hole stopper and short tube (for b), 
thermometer. 

a. Wind enough copper wire around a small lump of ice to make 
it sink in water, slip it into a large test tube nearly full of water, and 
heat the water quickly near the surface. Observe the effect on the 
ice. What does this experiment show about the conducting power 
of water? 

b. Fill a large test tube full of water, and insert a one-hole rubber 
stopper fitted with a short glass tube. Attach the test tube holder 
and heat the water slowly. Observe any change in the volume as 
the temperature of the water rises. Then cool the water by hold¬ 
ing the test tube in a stream of running water, and observe any change 
in the volume. What does this experiment show about the effect 
of heat on the expansion and contraction of water? 

c. Fill a large test tube half full of water, clamp it in an upright 
position to an iron stand, and heat the water to boiling. Hold the 
bulb of a thermometer in the escaping steam and note the highest 
temperature reached. Slowly lower the thermometer until the bulb 
touches the boiling water, note the highest temperature, and then 
remove the thermometer. Compare the two maximum readings. 
What is the boiling point of the water? What is the normal boiling 
point ? 

d. Fill a 250 cc. bottle half full of water, drop in several pieces of 
ice, and shake for two or three minutes. Insert the thermometer 


WATER — HYDROGEN PEROXIDE 


41 


until the bulb is immersed, and after a minute or two note the lowest 
temperature. Apply the questions in c to the freezing point. 

Experiment 30 — Water Vapor and Steam 

(Demonstration Experiment) 

Apparatus. — As in Fig. 40, page 64, author’s Practical Chemistry. 

Proceed as in § 71 , next to last paragraph. 

Proceed as in § 73 , second paragraph. 

Required Exercises. — 1. Describe the experiment. 

2. State the result briefly. 

3. What is steam? 

4. How does water vapor differ from steam? 

5. Sketch the apparatus. 

Experiment 31 — Water Vapor Exerts a Pressure 

(Demonstration Experiment) 

Apparatus. — As in Fig. 41, page 66, author’s Practical Chemistry. 
Required Exercises. — 1. Describe the experiment. 

2. State the result briefly. 

3. To what was the result due? 

4. What change in the result would a higher temperature have made? 
A lower temperature ? 

5. Sketch the apparatus. 

Experiment 32 — Some Chemical Properties of Water 

Materials. — Sodium, potassium, zinc sulphate solution, sulphur, calcium 
oxide. 

a. (See Caution in Exp. 21.) Fill an evaporating dish half full 
of water. Obtain three or four small pieces of sodium from the 
Teacher; place a mortar over the sodium until needed. 

Drop a piece upon the water in the dish, stand back and observe 
the result, waiting for the slight explosion before approaching the 
dish again; repeat with the rest of the sodium, piece by piece. 

When the chemical action is over, stand the dish on a gauze-covered 
ring attached to an iron stand, and heat until the water is entirely 
evaporated. Meanwhile proceed with c. Make three tests of the 
residue. (1) Moisten the end of a glass rod, touch the residue with 
it, and then draw this end across a piece of moistened red litmus 


42 EXPERIMENTS IN PRACTICAL CHEMISTRY 


paper. Observe the change in color of the litmus paper; this change 
is caused by hydroxides — sodium hydroxide in this case. 

(2) Moisten the looped end of a clean test wire (Fig. 29), touch 
the residue with it, and hold the end of the wire in the flame. Ob¬ 
serve the color of the flame; it is caused by the sodium in the resi¬ 
due. The production of this color is a test for sodium. 

(3) Dissolve the rest of the residue in 10 cc. of water, pour a 
little of the solution into a test tube, add a few drops of zinc sul¬ 
phate solution, and shake. Observe the result. Now pour the rest 
of the solution into the test tube and shake well. Observe the 
result. This is a test for the hydroxide part of sodium hydroxide. 

o*-- fc— _ ) 


<=>-"- y / ^ 

Fig. 29. — Test wires — platinum (upper), nichrome (lower) 

b. Teacher’s Experiment. — Remove a lump of potassium from 
the bottle, cut off two or three small slices, and put the rest back in 
the bottle. Fill a pneumatic trough nearly full of water. Throw 
a piece on the water and stand back until the slight explosion is heard 
Note the result, especially the difference from sodium. Repeat with 
the rest, piece by piece. Test the water (near the surface) with red 
litmus paper. State the result. Compare with the test in a (1). 
What substance is in the water? 

c. (1) Put a little water in a bottle. Set fire to a small piece of 
sulphur in a deflagrating spoon and lower the burning sulphur into 
the bottle. Let it burn a minute or two, then extinguish the flame 
by dipping the spoon into the water. Remove the spoon, cover the 
bottle with the hand, and shake well. Dip a glass rod into the liquid, 
draw the moistened end across a piece of blue litmus paper, and ob¬ 
serve the change in color. This change in the color of blue litmus 
is caused by acids; in this case the acid is sulphurous acid, which was 
produced by the combination of the sulphur oxide and water. 

(2) Boil a small piece of calcium oxide with a little water in a test 
tube. Test with red litmus paper as in (1). If the result is indiffer¬ 
ent, put the paper in the test tube and shake well. Observe the re¬ 
sult in a minute or two. Compare with (1). 

Required Exercises. — 1. State briefly the essential chemical change 
that took place in c (1) and (2). 

2. State these chemical changes as equations (using the names of the 
substances). 









WATER — HYDROGEN PEROXIDE 


43 


Experiment 33 — Solubility of Gases in Water 

a. Fill a bottle half full of water, close with the hand and shake 
vigorously several minutes. Fill a test tube nearly full and warm the 
test tube gently. What is the immediate evidence of dissolved gas? 
What effect has increased heat on the dissolved gas ? 

b. Heat the following in separate test tubes as in a : Faucet water, 
ammonium hydroxide, dilute hydrochloric acid. State in each case 
the evidence of dissolved gas. (Note. — As soon as the observation is 
made, pour the liquids down the sink and flush it well with water.) 

Answer: i. Does distilled water contain dissolved gases? 

2. What gas does soda water contain? 

3. In which are gases more soluble, hot or cold water? 

Experiment 34 — Solubility of Liquids in Water 

Materials. — Alcohol (ethyl or methyl), gasolene, glycerin, aniline, ether, 
carbon tetrachloride. 

a. To a test tube one-third full of water add a little alcohol and 
shake. Is there evidence of solution ? Add a little more and shake 
well. Add a third portion and shake. Is there still evidence of 
solution? Draw a conclusion as to the mutual solubility of alcohol 
and water. 

b. Repeat a, using successively gasolene, glycerin, aniline, ether, 
and carbon tetrachloride. Observe the results in each case and con¬ 
clude accordingly. 

c. Tabulate the results of a and b under the headings Mutual 
Solubility, Limited Solubility, Very Slight Solubility. 

Experiment 35 — Solubility of Solids in Water 

Materials. — Sand, calcium sulphate, sodium chloride, potassium per¬ 
manganate, sodium hydroxide (solid), calcium carbonate (powder). 

Put about 1 gm. of the substances in separate test tubes, add 10 cc. 
of water, and stand the tubes in a rack. Shake well and note the 
evidence of solubility. In case of doubt, let the solid settle, and 
transfer half of the clear liquid to an evaporating dish by pouring 
it down a glass rod (Fig. XIV), and evaporate by heating the dish 
on a gauze. What is the final evidence of solubility ? 

Tabulate the difference in solubility as below, using the terms Very 
soluble, Moderately soluble, Slightly soluble, Insoluble. 


44 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Difference in Solubility of Solids 


Solvent —10 cc. 

Solid — i gm. 

Result 


1. Sand 

1. 


2. Calcium Sulphate 

2. 

Water at temperature 

3. Sodium Chloride 

3 - 

of Laboratory 

4. Potas. Permanganate 

4- 


5. Sodium Hydroxide 

5- 


6. Calcium Carbonate 

6.. 


Experiment 36 —Effect of Heat on the Solubility of Solids 

Materials. — About 5 gm. each of powdered copper sulphate and potas¬ 
sium chlorate, calcium hydroxide solution for c. 

a. Label two test tubes, I, II. Put 10 cc. of water into each. 
To I add 1 gm. of powdered copper sulphate, and to II add 1 gm. of 
powdered potassium chlorate. Shake each test tube, and then allow 
them to stand undisturbed until the solid settles. Is there evidence 
of solubility in each case? (Save for b.) 

b. Heat I, and add gradually 2 gm. of powdered copper sulphate. 
Does it all dissolve? Heat II and add 2 gm. of powdered potassium 
chlorate. Does it dissolve? Add the rest of each solid to the re¬ 
spective. tubes, and heat (but do not boil). What effect has in¬ 
creased heat on the solubility of the solids? (Save for Exp. 38.) 

c. Fill a test tube half full of clear calcium hydroxide solution, 
and heat it to boiling. Observe the result. Compare with the cold 
solution. What effect has increased heat on the solubility of cal¬ 
cium hydroxide? How does the result differ from b? 

Experiment 37 — Effect of Shape on the Solubility of a Solid 

Material. — Crystallized alum. 

Apparatus. — 2 large test tubes fitted with corks. 

Weigh about 2 gm. of crystallized alum (in one lump, if possible) 
on the scales, and counterpoise it with a second quantity of equal 
weight. Pulverize the latter in a mortar. Put each in a test tube, 
add 25 cc. of water, and insert the cork. Note the time. Shake the 
tubes gently until the powder has dissolved. Note the time again. 
Estimate the amount of alum left in the other tube, or, if time per¬ 
mits, continue to shake at intervals until the solid has dissolved, and 
note the time again. 
















WATER — HYDROGEN PEROXIDE 


45 


Compare the times required to dissolve the powder and the crystal. 
Why does dissolving occur faster in one case than in the other? 

Experiment 38 — Saturated Solutions 

Materials. - — Solutions from Exp. 36 b, sodium chloride. 

Apparatus. — Large flask or bottle, hydrometer (specific gravity — direct 
reading) for liquids heavier than water, tall jar (e.g. a 250 cc. graduated 
cylinder). 

a. If the test tubes with contents from Exp. 36 b were saved, use 
them; if not, prepare new solutions. 

If the contents of the test tube is not liquid, add a little water, and 
heat gently until the solid dissolves. Cool each solution quickly 
by holding the lower end of the test tube in a stream of water. Are 
crystals formed? Are they formed at once? Are they large or 
small ? 

b. Wipe each test tube dry and heat gently until 
the liquid is clear. Stand the tubes in a rack, and let 
each solution cool slowly and stand undisturbed 
until the next laboratory period. Observe the result. 

Compare the size and general shape of the crystals 
with those formed in a. 

c. Demonstration Experiment. — Prepare a satu¬ 
rated solution of sodium chloride by shaking about 
100 gm. of fine salt with 275 cc. of water in a flask 
or bottle until no more salt dissolves. Let the 
undissolved salt settle and carefully pour the clear 
solution into the tall jar. Take the temperature. 

Let the hydrometer sink carefully into the solution. 

When the instrument becomes still, read the num¬ 
ber on the scale (on the stem) that is level with 
the surface of the liquid (Fig. 30). This number is 
the specific gravity of the solution. Compare the 
concentration with that read from the solubility 
curve shown in Fig. 43 on page 72 of the author’s 
Practical Chemistry 




Fig. 30. — Find¬ 
ing the spe¬ 
cific gravity 
of a solution 
with the hy¬ 
drometer 


Experiment 39 — Solubility of a Given Solid 

Object. — To find the number of grams of potassium dichromate dissolved 
in 100 gm. of water. 

Material. — Potassium dichromate solution (concentration known only 
to Teacher). 

Apparatus. — Water bath as in Fig. 31. 





46 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Copy the form of Record in the notebook. Enter all weights in 
the proper place as soon as weighings are made. 

Weigh an evaporating dish on the balance, and enter the weight 
at once in the Record in the notebook. Obtain from the Teacher 
exactly 25 cc. of the potassium dichromate solution. Pour the solu¬ 
tion into the weighed dish. Weigh the dish and contents, and record 
the weight. 


Record 


Weight of dish and solution. gm. 

Weight of dish. gm. 

Weight of solution. gm. 

Weight of dish and solid — I gm. II. gm. Ill. gm. 

Weight of dish. gm. 

Weight of solid. gm. 

Weight of water ( i.e . solution — solid). gm. 

Weight of solid dissolved in 100 gm. of water. gm. 


Stand the dish on a water bath and evaporate 
the solution to dryness (Fig. 31). 

Complete the evaporation by transferring 
the dish to a gauze-covered ring and heating 
intensely. When the dish is cool, weigh, and 
record the weight. Heat again on the gauze, 
cool, and weigh; if the two weights are the 
same (or nearly so), accept the first weighing, 
but if the weights are considerably different, 
heat intensely (but do not melt the solid), cool, 
and weigh a third time. 

Complete the entries in the Record. Cal¬ 
culate the weight of the solid dissolved in 100 
gm. of water. Submit the result to the 
Teacher before throwing away the contents of 
the dish. 

Experiment 40 — Formation of Crystals 

Material. — Powdered alum or borax. 

Apparatus. — Thread, lens. 

Prepare a hot, concentrated solution of alum or borax by boiling 
about 10 gm. of alum or 5 gm. of borax in 10 cc. of water in a large 
test tube. Pour the solution into an evaporating dish (or a 



Fig. 31. — Water bath 
for evaporating a 
solution to dryness 




















WATER — HYDROGEN PEROXIDE 


47 


beaker). Suspend a piece of thread in the solution (as in Fig. 32). 
Stand the whole aside to crystallize. 


Examine at intervals, and when well¬ 
shaped crystals have formed on the thread, 
remove the thread. Dry the crystals 





carefully with filter paper. Examine 
them, using a lens if the crystals are 
small, and observe the properties, partic¬ 
ularly the shape, luster, and color. Test 
a crystal for water of crystallization. 




Required Exercises. — 1. Describe this 
experiment. 

2. What is the name of the shape of a 
typical alum crystal? (A borax crystal?) 

i 



3. What term describes the luster? 

4. Do the crystals contain water of crystal¬ 
lization ? Is the amount conspicuously large ? 

Fig. 32. — Crystallizing 
alum 


Experiment 41 — Testing for Water of Crystallization 

Materials. — Sodium carbonate, potassium dichromate, ferrous sulphate, 
borax, barium chloride, zinc sulphate, sodium sulphate, calcium sul¬ 
phate, sodium chloride, potassium nitrate, sugar, magnesium sulphate, 
potassium bromide. 

Test several of the substances for water of crystallization by heat¬ 
ing a dry specimen in a dry test tube inclined so that the open end 
is the lower. Observe in each case the change in appearance of the 
solid during the heating, relative amount of water liberated (if appre¬ 
ciable), and appearance of the residue. State each result. 

Experiment 42 — Per Cent of Water of Crystallization 

Object. — To find the weight of water lost by heating a weighed amount 
of crystallized copper sulphate, and to calculate the per cent of watei 
of crystallization. 

Material. — Crystallized copper sulphate (powdered). 

Copy the form of Record, as given below, in the notebook, and 
enter all weights as soon as the weighing is completed. 

Clean and dry an evaporating dish and weigh it to a decigram on 
the scales. Put about 10 gm. of powdered copper sulphate in the 
dish and weigh to a decigram. Record the weight at once. 













48 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Record 


Weight of dish and copper sulphate before heating . . . gra. 

Weight of dish .. gm. 

Weight of copper sulphate. gm. 

Weight of dish and copper sulphate before heating . . . gm. 

Weight of dish and contents after heating..gm. 

Weight of water of crystallization. gm. 

Per cent of water of crystallization. per cent 


Stand the dish with its contents on a gauze-covered ring attached 
to an iron stand, heat gently for five or ten minutes, and then intensely 
until the substance becomes a gray powder. Do not touch the sub¬ 
stance, and take special pains not to lose any. Cool slowly and weigh 
as before. Record the weight at once. Complete the entries in the 
Record, and calculate the per cent of water of crystallization. Sub¬ 
mit the result to the Teacher before throwing away the contents of 
the dish. 


Experiment 43 — Anhydrous Compounds 

Materials. — Hydrated (crystallized) copper sulphate and cobalt chloride. 

a. Pulverize a little hydrated copper sulphate and note the color. 
Put it in a test tube, hold the tube horizontal, and spread the powder 
along the tube. Hold the mouth of the tube slightly lower than the 
other end, and heat gently. Begin to heat at the closed end and 
move the tube in the flame so that all the liberated water is finally 
driven from the tube. Note the color of the anhydrous solid. Let 
the tube cool. Meanwhile do b. 

When the tube is cool, cautiously add a little water, and let it run 
down upon the solid. What effect does the water have on the color 
of the solid ? 

b. Proceed as in a, using hydrated cobalt chloride. 

Answer: i. What is the difference between a hydrated and an anhydrous 
compound ? 

2. What is the color of hydrated copper sulphate? Dehydrated? An¬ 
hydrous ? 

3. As in 2 for cobalt chloride. 

Experiment 44 — Efflorescence 

Materials. — Sodium carbonate, sodium sulphate, ferrous sulphate, potas¬ 
sium ferrocyanide, barium chloride, magnesium sulphate. 









WATER — HYDROGEN PEROXIDE 


49 


Put a fresh, or a recently broken, crystal of several of the substances 
on a piece of filter paper, and label each. Let them remain exposed 
to the air for an hour or more. Describe any marked change in the 
appearance. 

Answer: i. What does the change, if any, show about the air? About 
the crystal? 

2. To what is the change due? 


Experiment 45 — Deliquescence 

Materials. — Sodium hydroxide, calcium chloride, potassium hydroxide, 
magnesium chloride, table salt, zinc chloride, potassium carbonate, 
sodium nitrate. 

Proceed and answer as in Exp. 44. 


Experiment 46 — Efflorescence and Deliquescence 

(Demonstration Experiment) 


Materials. — Crystallized copper sulphate, concentrated sulphuric acid, 
sodium hydroxide. 

Apparatus. — 4 test tubes fitted with corks, thread, copper or iron wire. 


a. Select two pieces of crystallized copper sulphate which will 
just slip into a test tube. Tie a thread around each piece. Put 10 cc. 
of water into one test tube, and 10 cc. of con¬ 
centrated sulphuric acid into the other, taking 
care not to leave any drops on the inside of the 
test tube. Hang a piece of the solid in each 
test tube and insert the cork tightly (Fig. 33); 
smear a little vaseline around the upper edge 
of the test tube containing the acid to make 
the joint air-tight. Let the test tubes stand 
in the rack undisturbed for several hours (or 
until the next laboratory period), and then ex¬ 
amine each solid. Compare them with each 
other and with a sample of the original substance. 

State the change, if any, in each case; state 
also the degree of change, if possible. Why do 
the changes differ in degree? Explain. 

b. Proceed as in a, using sodium hydroxide. Wind the wire around 
the solid and attach the wire to the thread. Observe, answer, and 
explain as in a. 


Fig. 33. — Solid sus¬ 
pended in a closed 
test tube to show 
efflorescence and 
deliquescence 




50 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 47 — Supersaturation 


Material. — Sodium thiosulphate. 

Apparatus. — Test tube fitted with a cork. 

Fill a test tube half full of crystallized sodium thiosulphate and 
add 2 or 3 cc. of water. Warm slowly until all the solid has dissolved. 
Pour the solution into a warm, clean, dry test tube, insert a cork, 
and let it stand undisturbed until cool. Note the change in the 
solution, if any. Drop in a small crystal of sodium thiosulphate and 
watch for a definite change. What happens? Observe and state 
the final result. 

Answer: i. What is the difference between a saturated and an unsat¬ 
urated solution? 

2. How could you determine whether a cold solution is saturated, un¬ 
saturated, or supersaturated? 


Experiment 48 — Qualitative Composition of Water 

(Demonstration Experiment) 


Materials. — Chlorine water (see Exp. 6o), joss 
stick. 

Apparatus. — Chlorine tube (tube about i m. long 
closed at one end). 



Fill the tube with chlorine water, cover the open 
end with the thumb or finger, invert the tube, and. 
immerse the open end in a mortar or an evapo¬ 
rating dish, which should be nearly full of chlorine 
water (Fig. 34). Clamp the tube in an upright 
position, and stand the whole apparatus where 
it will receive the direct sunlight for several 
hours. Bubbles of gas will collect at the top. 

When sufficient gas for a test has collected, 
unclamp the tube, cover the open end with the 
thumb or finger, invert, and put a glowing joss 
stick into the gas. Repeat as long as any of the 
gas remains. State the result. What is the gas ? 


p IG 24._Appara- Required Exercises (Review). — 1. What evi- 

tus for showing dence does the interaction of water and sodium give 
that oxygen is a about the composition of water? 
constituent of 2. Apply Exercise 1 to the burning of hydrogen, 

water 3. Apply Exercise 1 to the reduction of copper oxide. 











WATER — HYDROGEN PEROXIDE 


51 


Experiment 49 — Electrolysis of Water 

(Demonstration Experiment) 


Materials. — Sulphuric acid, joss stick, taper. 
Apparatus. — Hofmann apparatus. 


Fill the Hofmann apparatus (Fig. 35) with water containing 10 per 
cent of sulphuric acid, so that the water in the 
reservoir tube stands a short distance above the 
gas tubes after the stopcock in each has been 
closed. Connect the platinum terminal wires 
with a battery of at least three cells (or a street 
current reduced by suitable resistance). 

As the action proceeds, small bubbles of gas 
rise and collect at the top of each tube. Allow 
the current to run until the smaller volume of gas 
is 8 to 10 cc. 

Measure the height of each gas column. As¬ 
suming that the tubes have the same diameter, 
the volumes are in approximately the same ratio 
as their heights. How do the volumes com¬ 
pare? 

Test each gas. a. Open the stopcock of the 
tube containing the smaller quantity of gas long 
enough to allow the water (or air) to run out 
of the glass tip, and then close it immediately. 

Let out a little gas upon a glowing joss stick, 
and observe the result. Close the stopcock as 
soon as the result is seen. What is the gas? 

Repeat, if gas is available. 

b. Open the other stopcock long enough to 
force out the water (or air) in the glass tip and 
then close it. Open the stopcock again, let out 
a little gas slowly, hold a lighted match for an instant at the 
end of the tip, and immediately thrust a taper into the small and 
almost colorless flame. Watch for a change in the taper. Close 
the stopcock as soon as the change is seen. What is the gas ? 



Fig. 35. — Hofmann 
apparatus for 
the electrolysis 
of water 


Required Exercises. — 1. Describe this experiment and sketch the 
apparatus. 

2. What does this experiment show about the composition of water? 

3. Compare answer to 2 with answers at the end of Experiment 48. 

















52 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 50 — Properties of Hydrogen Peroxide 

Materials. — Hydrogen peroxide, manganese dioxide, potassium perman¬ 
ganate solution, lead nitrate solution, hydrogen sulphide (or ammonium 
sulphide) solution, joss stick. 

a. Heat a little hydrogen peroxide, and observe the result. Now 
add a little powdered manganese dioxide to the heated liquid, and 
observe the result. Test the escaping gas for oxygen. What is the 
result ? 

b. Add several drops of potassium permanganate solution to a 
little hydrogen peroxide, and observe the result. Is a gas evolved? 
If so, test it with a glowing joss stick. If not, add more potassium 
permanganate solution, and then test. What is the gas? 

c. Prepare a little lead sulphide by adding a few drops of hydro¬ 
gen sulphide (or ammonium sulphide) solution to dilute lead nitrate 
solution. Note the color of the lead sulphide. Shake well, add 
hydrogen peroxide, and warm gently. Observe the change in color. 
To what is the change due? 

d. Examine the inner end of the cork stopper of a bottle of hydro¬ 
gen peroxide. Explain the color. 

LAWS OF CONSTANT COMPOSITION AND 
MULTIPLE PROPORTIONS 

(Practical Chemistry, pp. 87-100, §§ 96-109) 

Experiment 51 — Law of Constant Composition 

Object. — To find the weight of oxygen that combines with a definite weight 
of magnesium. 

Material. — Powdered magnesium. 

Apparatus. — Porcelain crucible and cover, triangle. 

Copy the form of Record (see below) in your notebook and 
enter each weight as soon as the weighing is made. 

Clean and dry the crucible and cover, and weigh both together 
accurately on the balance. (See Introduction, § 8, for directions 
about weighing.) Enter the weight in the notebook. Put from 
0.4 to 0.5 gm. of magnesium in the crucible, and weigh (with cover) 
exactly the amount taken. Enter the weight. In carrying the cru¬ 
cible to and from the balance, it should be placed in the crucible 
block (Fig. 37). 

Support the covered crucible as in Fig. 36, and heat for five min- 


LAW OF CONSTANT COMPOSITION 


53 



utes with a flame which touches the bottom of the crucible. Grasp 
the cover firmly by the ring with the clean 
forceps, cautiously lift it, and if the magnesium 
glows, cover the crucible instantly. Repeat 
this operation at frequent intervals, gradually 
increasing the heat, until the glow ceases to 
spread through the mass. Then adjust the 
cover so that a small opening is left between 
the cover and the crucible, and heat intensely 
for ten or fifteen minutes. If the contents has 
ceased to glow, heat the crucible, uncovered, 

for five or ten min¬ 
utes. 

Cool the cru¬ 
cible gradually. 

When cool, weigh, 
and enter this 
weight as I in the 



Fig. 37. — Crucible block 
for carrying a crucible 


Fig. 36. — Covered 
crucible supported 
on a triangle 


proper place. 

Heat the uncovered crucible again intensely for five or ten minutes. 
Cool, and weigh as before; enter this weight as H. If the weight 
is not the same, submit the result to the Teacher. 


Record 

Wt. of crucible, cover, and magnesium. gm. 

Wt. of crucible and cover. gm. 

Wt. of magnesium. gm. 

Wt. of crucible, cover, and magnesium oxide I gm., 

II gm., Ill. gm. 

Wt. of crucible and cover. gm. 

Wt. of magnesium oxide. gm. 

Wt. of magnesium oxide. gm. 

Wt. of magnesium. gm. 

Wt. of oxygen. gm. 


From the weights of the magnesium and the oxygen, calculate the 
ratio in which the two elements combined. Submit the result to 
the Teacher before throwing away the contents of the crucible. 

Note. — The crucible, if blackened, can be cleaned by heating a little 
sodium hydroxide solution in it and then washing thoroughly with 
water. 
























54 EXPERIMENTS IN PRACTICAL CHEMISTRY 

Experiment 52 — Law of Multiple Proportions 

Object. — To find the weight of oxygen liberated by heating known weights 
of potassium chlorate and potassium perchlorate. 

Materials. — Powdered potassium chlorate and potassium perchlorate. 
Apparatus. — As in Exp. 51. 

Copy the form of Record (see below) in your notebook and 
enter each weight as soon as the weighing is made. 

I. (For one section of the class.) Clean and dry the crucible and 
cover, and weigh both together accurately on the balance. Put in 
the crucible about 1.5 gm. of dry powdered potassium chlorate and 
weigh (with cover) the exact amount taken. 

Support the covered crucible as in Fig. 36. Heat with a flame 
about an inch below the bottom of the crucible. The potassium 
chlorate melts, begins to decompose, and the oxygen bubbles through 
the molten mass. Heat about fifteen minutes. Then lower the 
crucible or raise the burner, until the flame covers the bottom of the 
crucible. Heat about twenty minutes. 

If the flame is too high, the potassium chlorate may spatter and 
adhere to the inside of the cover. Remove the cover with the forceps 
occasionally, and if it is coated with potassium chlorate, replace it, 
and let the crucible cool somewhat. Remove the cover, lay it (ring 
side down) on a piece of paper on the crucible block (Fig. 37), and 
loosen the thin layer with a pin. Grasp the cover with the forceps, 
turn out the pieces upon the paper, and finally scrape them from the 
paper into the crucible. 

When there is no danger of loss by spattering, remove the cover, 
lay it (ring side down) on the crucible block, and heat the crucible 
for twenty or thirty minutes. 

Let the crucible cool gradually, and when cool, weigh the crucible, 
cover, and contents, as before. Record the weight as I in the proper 
place. 

Heat the uncovered crucible again strongly for five or ten minutes, 
then cool, weigh as before, and record as II. If the weight is the 
same as after the first heating, proceed with the calculation; if not 
the same, heat, weigh again, and record as III. 

From the weights of the potassium chlorate and the oxygen, calcu¬ 
late the per cent of oxygen in potassium chlorate. Do this before 
throwing away the contents of the crucible. 


LAW OF CONSTANT COMPOSITION 


55 


Record 


Wt. of crucible, cover, and potassium chlorate. gm. 

Wt. of crucible and cover..gm. 

Wt. of potassium chlorate. gm. 

Wt. of crucible, cover, and contents before heating .... gm. 

Wt. of same after heating I gm., II gm., Ill..gm. 

Wt. of oxygen in potassium chlorate. gm. 

Per cent of oxygen in potassium chlorate. 


II. (For one section of the class.) Proceed as in I, using dry potas¬ 
sium perchlorate. Enter all weights in the Record, and calculate 
the per cent of oxygen in potassium perchlorate. 

III. (For the class.) Calculation. (See § 99 in the author’s 
Practical Chemistry.) According to the law of multiple proportions, 
if we adopt a fixed weight of one part of a compound as a basis, and 
express the composition in terms of this weight, then the weights 
of the other part can be expressed in a simple multiple relation. Let 
us take potassium chloride as the fixed part and oxygen as the multi¬ 
ple part. 

Our problem is to find the small whole numbers which show the 
simple multiple relation between the weights of oxygen in the two 
compounds potassium chlorate and potassium perchlorate. 

a. First, we subtract each per cent of oxygen from 100 (per cent) 
to find the per cent of the potassium chloride part of each compound. 
Thus, if we take the exact per cents of oxygen, the per cents of potas¬ 
sium chloride are 

60.82 ( i.e 100 — 39.18) and 53.79 ( i.e . 100 — 46.21) 

b. Second, we adopt 1 as the fixed weight of the potassium chlo¬ 
ride part. And we reduce each per cent of potassium chloride to 1, 
thus, 

60.82 -f- 60.82 = 1 and 53.79 4 - 53.79 = 1 

c. But in order to keep the correct proportion of potassium chloride 
to oxygen (found by our experiments), we must also divide each per 
cent of oxygen by the corresponding number used in b. Thus, 

39.18 4 - 60.82 = 0.644 and 46.21 -T- 53.79 = 0.859 

These numbers (0.644 and 0.859) represent the weights of oxygen, 
if the weight of potassium chloride were 1 in each compound. 

d. Our final step is to find the small whole numbers which cor¬ 
respond to 0.644 an d 0.859. If we divide 0.644 by 0.859 and express 
the quotient as a common fraction, we obtain f. This means that 
0.644 and 0.859 are in the same relation as 3 and 4. This means that 










56 EXPERIMENTS IN PRACTICAL CHEMISTRY 


the weights of oxygen in the two compounds are in the simple multi¬ 
ple relation 3: 4. 

Note. — The per cents of oxygen obtained by individual experiments 
will probably not give numbers which are in exactly the ratio 3: 4, but a 
class average is usually very near 3:4. 


NITROGEN — AIR 

(Practical Chemistry, pp. 102-113, §§ 110-131) 

Experiment 53 — Preparation and Properties of Nitrogen 

Materials. —Ammonium chloride, sodium nitrite, joss stick, iron thread, 
sulphur. 

Apparatus. — As in Fig. 38. 

I. Preparation. — Weigh 8 gm. of ammonium chloride and 10 gm. 
of sodium nitrite, put them in the flask, add 50 cc. of water, and 
shake well. Arrange the apparatus, as in Fig. 38, to collect the gas 

over water. Fill the bottles 
with water and invert one in 
the trough. Have two more 
bottles ready to replace this 
one. Fill the cup of the 
dropping funnel with water, 
and then ask to have the ap¬ 
paratus inspected by the 
Teacher. 

Heat the flask gently with 
a low flame, and as soon as 
the nitrogen bubbles regularly 
through the water, slip the 
bottle over the hole in the 
support. Heat gently, but 
enough to keep the gas 
bubbling slowly through the 
Fig. 38. — Apparatus for preparing water. Collect three bottles 
nitrogen of nitrogen. 

Caution. — If the mixture 
in the flask begins to froth or the gas comes off too rapidly, re¬ 
move the flame and let in a little water; if it continues to froth, 
pinch the clamp to let out the excess of gas. As soon as the froth¬ 
ing lessens, close the clamp and heat gently. Remove the end of the 



















NITROGEN — AIR 


57 


delivery tube from the water as soon as the last bottle of nitrogen 
has been collected. Proceed at once with II. 

II. Properties. — a. Thrust a blazing joss stick into a bottle of 
the gas. Observe and state the result. 

b. Put a piece of sulphur in a deflagrating spoon, light the sulphur, 
lower it into a bottle of nitrogen, and keep it there about half a minute. 
Observe the result. Withdraw, and observe the result. If the sul¬ 
phur is still burning, repeat. State the results. 

c. Wind one end of a copper wire around a wad of iron thread, 
heat a few strands, and quickly thrust the glowing iron into a bottle 
of nitrogen. Observe and state the result. 

Required Exercises. — i. Describe briefly the preparation of ni¬ 
trogen. 

2. Sketch the apparatus. 

3. Compare the characteristic properties of nitrogen with those of oxygen 
found by similar experiments. 

Experiment 54 — Transformation of Combined Nitrogen 
into Ammonia (Test for Combined Nitrogen) 

Materials. — Albumin, soda-lime, gelatin, meat, peas, beans, flour, bread, 
fertilizer. 

a. Put a little egg albumin in a test tube and add about five times 
its bulk of soda-lime. Mix by shaking. Heat gently (in the hood) 
and hold a piece of wet red litmus paper in the escaping smoke. Ob¬ 
serve and state the change in the color of the litmus paper. (One 
product of the interaction is ammonia gas, but its odor is usually 
masked by the burning albumin. The nitrogen needed for the ammo¬ 
nia comes from the compound (albumin in this case).) 

b. Proceed as in a, using gelatin, meat, peas, beans, flour, bread. 
State each result. 

c. Proceed as in a, using samples of fertilizers. State each re¬ 
sult. 


Experiment 55 — Per Cent of Oxygen in Air 

Object. — To find the volume of oxygen absorbed from a measured volume 
of air. 

Materials. — Solutions of pyrogallic acid (10 per cent) and sodium hy¬ 
droxide (50 per cent). 

Apparatus. — As in Fig. 39; pneumatic trough half full of water at room 
temperature, 250 and 25 cc. graduated cylinders. The bottle holds 


58 EXPERIMENTS IN PRACTICAL CHEMISTRY 


about 250 cc. and is provided with a tightly fitting one-hole rubber 
stopper through which passes a glass plug. The plug is made by clos¬ 
ing both ends of a glass tube about 10 cm. (4 in.) long, and should fit 
tight. 

Copy the form of Record as given below in your notebook and 
enter each volume as soon as the readings are made. 

First find the volume of the bottle. Fill the 
pneumatic trough with water and add hot water, if 
necessary, to raise the temperature to that of the 
room. Fill the bottle full of water from the pneu¬ 
matic trough. Push the stopper into the bottle as 
far as it will go, insert the glass plug until the inner 
end is flush with the inner surface of the stopper, 
and then draw a line around the stopper with a 
lead pencil to mark its position. Remove the plug 
and then the stopper carefully, to avoid loss of water. 
Pour water from the bottle into the 250 cc. graduate 
until the graduate is full (to the 250 cc. mark) or 
the bottle is empty; read the volume. If the bottle 
holds more than 250 cc., the rest of the water in the 
bottle may be poured into the 25 cc. graduate. Re¬ 
total volume of the bottle as shown below. 

Record 


a. Volume of bottle .. cc. 

b. Volume of original solution (total)..cc. 

c. Volume of air taken (a — b) . cc. 

d. Volume of final liquid.. cc. 

e. Volume of water which entered ( d—b ). cc. 

/. Per cent of water which entered (e -=-c). 


The per cent of entering water equals the per cent of gas absorbed. 
Therefore: — 

g. Per cent of oxygen in the sample of air. 

h. Per cent of nitrogen (100— g) . 

Measure exactly 10 cc. of pyrogallic acid in the 25 cc. graduate, 
and pour it carefully into the bottle. Measure also exactly 20 cc. 
of sodium hydroxide solution, and pour it into the bottle. (Cau¬ 
tion. — The sodium hydroxide solution is corrosive. Do not spill 
it on the hands or clothing.) Insert the rubber stopper (with its 
plug) quickly to the proper mark. 

Shake the bottle vigorously for a few minutes, and then invert it 



Fig. 39. — Ap¬ 
paratus for 
finding the 
per cent of 
oxygen in air 













NITROGEN — AIR 


59 


and watch the surface of the liquid for bubbles of air, which will enter 
if the apparatus leaks. If a leak is detected, ask the Teacher for 
directions before proceeding. If the apparatus is tight, continue the 
shaking for about half an hour. During this operation the oxygen 
is absorbed by the solution. 

Place the bottle on its side beneath the water in the pneumatic 
trough, inclining it slightly so that the lower edge of the bottle rests 
upon the bottom of the trough and the hole in the stopper is beneath 
the surface of the water. With one hand grasp the bottle firmly by 
the neck and stopper, and with the other gradually pull out the plug 
to let the water run in. Water will run in quickly to fill the space 
left by the oxygen. Take care not to pull out the stopper and not 
to let any of the solution run out. Be sure also to keep the hole in 
the stopper constantly beneath the surface of the water. After the 
water has stopped running in, lift out the bottle, and measure care¬ 
fully the volume of the liquid in the bottle by pouring it into a gradu¬ 
ate. Complete the entries in the Record. 

Note. — This experiment disregards the argon and carbon dioxide in air. 


Experiment 56 — Water Vapor in Air 

Material. — Calcium chloride or sodium hydroxide. 

Place a piece of calcium chloride or sodium hydroxide on a glass 
plate or a block of wood, and let it remain exposed to the air for an 
hour or more. Observe and state the result. How does this experi¬ 
ment show that air contains water vapor? 


Experiment 57 — Carbon Dioxide in Air 

Materials. — Calcium hydroxide and barium hydroxide solutions. 
Apparatus. — Air blast or suction apparatus (for b). 

a. Pour 25 cc. of calcium hydroxide solution into a bottle, and let 
it stand exposed to the air for an hour or more. Examine the sur¬ 
face of the liquid. State and explain the change. 

b. Optional. Force, or draw, air through a bottle half full of 
clear barium hydroxide solution until the liquid is conspicuously 
changed. Describe and explain the change. 

Answer: 1. What do a and b show about carbon dioxide in air? 

2. What does b show about the relative amount (large or small) ? 


6o EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 58 — Testing Air 

Materials. — As in Exps. 56, 57. 

Apparatus. — As in Exps. 56, 57. 

a. Apply Exps. 56 and 57 to the air in different parts of the school 
building. Start the tests at the same time to obtain comparable re¬ 
sults. 

b. Apply Exp. 56 to the air on several days. 

c. Apply Exp. 57 to the air in the laboratory, out doors, and in 
a recitation room which has just been vacated. Proceed with the 
testing as in a (this experiment). 

Tabulate the results of the whole experiment. 


CHLORINE — HYDROGEN CHLORIDE — HYDRO¬ 
CHLORIC ACID 


(Practical Chemistry, pp. 129-141, §§ 142-160) 

Experiment 59 — Chlorine — Short Method 


Materials. — Potassium permanganate, concentrated hydrochloric acid, 
wax taper, wad of iron thread, 2 pieces of copper wire about 15 cm. 
long, colored cloth, piece of newspaper, litmus paper (both colors), 
cotton, turpentine. 




Fig. 40. — Wads 
of cotton and 
iron thread for 
studying the 
properties of 
chlorine 


Caution. — Do not inhale chlorine. Do this 
experiment in the hood. 

I. Preparation. — Put 5 or 6 crystals of potas¬ 
sium permanganate in each of 4 bottles, add 3 to 
5 cc. of concentrated hydrochloric acid, shake, and 
cover the bottles with a piece of filter paper pressed 
down to form a loose cap. Chlorine is liberated 
and will slowly fill the bottles. When the color 
shows that a bottle is full, proceed at once with it 
as in II a. Use the other bottles when full as 
directed. 

II. Properties. — a. Remove the paper from a 
bottle of chlorine and thrust a blazing wax taper 
into the gas. Observe the result. Does the gas 
burn? Does the taper burn? What is the deposit 
inside the bottle? 

b. Using the same bottle as in a, hold a lighted 
wax taper just inside the bottle. Move it up and 
down slowly. If it goes out, relight it, and con- 




CHLORINE 


oi 


tinue. (If a taper is unsatisfactory, use a candle.) Observe the 
result. The wax consists mainly of compounds of hydrogen and car¬ 
bon. Is carbon detected? What becomes of the hydrogen?. (Sug¬ 
gestion. Compare with e below.) 

c. Twist one end of a copper wire around a wad of iron thread 
(Fig. 40), heat the wad for an instant in the flame, and quickly lower 
it into the second bottle of chlorine. Observe and describe the re¬ 
sult, especially the evidence of chemical action. 

d. Into the third bottle of chlorine hang (by a wire) pieces of 
colored cloth, litmus paper (both colors), newspaper, and paper con¬ 
taining writing in lead pencil, ink (black and red) — all moistened 
with water. Let the whole remain undisturbed for a few minutes 
(1 e.g . while e is being done). Then observe and describe the change. 
What is bleached? What is not bleached? 

e. Twist one end of the copper wire around a wad of cotton, satu¬ 
rate the cotton with turpentine (preferably warm), and lower the 
cotton into the fourth bottle of chlorine. Observe at once the for¬ 
mation of a white smoke and then the conspicuous result. What 
two products are formed by the interaction of chlorine and turpen¬ 
tine? 

Note. — As soon as II e has been completed, fill each bottle with water 
(in the hood) and pour the contents into a waste jar in the hood. 

Answer: 1. What is the color of chlorine ? Is this gas heavier or lighter 
than air? 

2. What compound was formed in c? 

3. Were the pencil mark and printing ink bleached in d? Why? 

4. Of what elements is the compound (or are the compounds) in turpen¬ 
tine composed ? 

5. What experiments show that chlorine is an active element? 

Experiment 60 — Chlorine — Long Method 

Materials. — Concentrated hydrochloric acid, 10 gm. of manganese diox¬ 
ide, and as in Exp. 59 (except potassium permanganate). 

Apparatus. — As in Fig. 41. A is a 250 cc. Erlenmeyer flask which stands 
on a gauze-covered ring ; the parts lettered B, C, D, E have been used 
in preceding experiments. F is a piece of stiff paper. If desired, the 
optional apparatus shown in Fig. 42 may be used. 

Caution. — As in Exp. 59. 

I. Preparation. — Slip the manganese dioxide into the flask. Ar- 


62 EXPERIMENTS IN PRACTICAL CHEMISTRY 


range the apparatus as shown in Fig. 41. Introduce enough concen¬ 
trated hydrochloric acid through the 
dropping tube B to cover the man¬ 
ganese dioxide. Heat the flask A gently 
with a small flame. Avoid heating so 
high that steam or hydrogen chloride is 
evolved. 

Chlorine is evolved, and passes into 
the bottle G , which should be removed 
when full (as seen by the color) and 
covered tightly with a piece of filter 
paper; the bottle may be easily re¬ 
moved by holding the paper cover F in 
one hand and pulling the bottle G aside, 
bending the whole delivery tube at the 
same time at the rubber connection D. 
If the evolution of gas slackens, introduce 
more acid. Collect four bottles, and pro¬ 
ceed at once as in II. 

II. Properties. — a to e as in Exp. 59 
a to e. 

Experiment 61 — Preparation of Chlorine by Electrolysis 

(Demonstration Experiment) 

Materials. — Sodium chloride, litmus solution, dilute 
hydrochloric acid. 

Apparatus. — As in Fig. 43. A is a small battery 
jar (or a beaker), the electrodes E and F are 
pieces of electric light carbon, and B is a piece of 
glass (or cardboard). A battery of at least six 
cells, or a reduced street current, is also needed. 

Fill A two-thirds full of dilute sodium chloride 
solution, add a few cubic centimeters of litmus 
solution, and just enough dilute hydrochloric acid 
to produce a faint pink color. Slip the partition 
into the vessel to lessen the diffusion of the Fig. 42. — Op- 
liquid. Insert the electrodes and connect them tiona.1 appara- 

with the battery. Turn on the current. Smell !" us P re P ar " 

cautiously of the gas evolved. Note its effect on mg C ° rme 
the litmus in this compartment. Turn off the current as soon as 
the observations have been made. 




Fig. 41. — Apparatus for 
preparing chlorine in large 
quantities 


























CHLORINE 63 

What is the gas? What is the change in color in the other com¬ 
partment? Explain it (in general terms). 

Experiment 62 — Chlorine Water 

Materials. — Chlorine water, litmus paper, colored cloth or paper, dark 
sponge, ink-stained and fruit-stained cloth, gold leaf. 

Prepare chlorine water by letting the gas 
bubble for fifteen minutes or more through a 
bottle or a test tube nearly full of water. 

a. Try the bleaching action of chlorine 
water on litmus paper, bright colored cloth or 
paper (that is not decolorized by water alone), 
a piece of dark sponge, ink-stained and fruit- 
stained cloth. State the results. 

b. Stand a test tube in the rack. Moisten 
the end of a glass rod, touch it to a small piece 
of gold leaf, hold the rod with the adhering 
gold leaf inside a test tube, and wash the gold 
leaf into the test tube by pouring about 15 cc. 
of chlorine water down the rod. Remove the rod. Warm the 
test tube gently and shake until a definite change in the gold is ob¬ 
served. State the final result. Into what has the gold been 
changed ? 

Answer: 1. What happens when chlorine water is exposed to the sun¬ 
light ? 

2. What two equations express the reactions in 1 ? 

Experiment 63 — Bleaching 

Materials. — Bleaching powder, dilute sulphuric acid, colored cloth for 
a; sodium hypochlorite solution, dilute hydrochloric acid, white cloth 
for b. 

Apparatus. — 3 Beakers (or bottles), glass rod. 

a. Demonstration Experiment. — Put a little bleaching powder 
into one beaker and add enough water to make a thin paste. Fill 
the second beaker one-third full of dilute sulphuric acid, and the re¬ 
maining beaker one-third full of water. 

Press the lower half of the colored cloth into the bleaching powder 
with the rod, and then into the acid, passing it back and forth several 
times. Finally wash the cloth thoroughly in the beaker of water, 
squeeze out the excess of water, and compare the cloth with the sam- 



Fig. 43. — Apparatus 
for preparing chlo¬ 
rine by electrolysis 















64 EXPERIMENTS IN PRACTICAL CHEMISTRY 


pie. Describe the change in the appearance of the cloth. If the 
change is not marked, try other kinds of cloth. 

b. Let a drop or two of ink fall from a fountain pen upon a piece 
of white cloth. Lay the cloth over an evaporating dish and pour a 
little sodium hypochlorite solution drop by drop upon the spot. Then 
pour slowly a little dilute hydrochloric acid upon the spot. Wash 
well with water and note the result. 

Experiment 64 — Hydrogen Chloride — Short Method 

Materials. — Sodium chloride, concentrated sulphuric acid, silver nitrate 
solution, litmus paper, ammonium hydroxide. 

Put a few grams of sodium chloride in a test tube, and add several 
drops of concentrated sulphuric acid. Hydrogen chloride is evolved. 

a. Hold a piece of moist blue litmus paper at the mouth of the 
test tube. Observe the result. 

b. Blow the (moist) breath across the mouth of the tube. Hold 
a piece of wet filter paper in the gas. Observe the result in each case. 
Explain it. 

c. Hold a glass rod moistened with ammonium hydroxide in the 
gas. Observe the result. What is the product? 

d. Moisten a clean glass rod with silver nitrate solution and hold 
it in the gas. Observe the result. What is the product? State 
the result. 

Experiment 65 — Hydrogen Chloride and Hydrochloric Acid 

Materials. — Sodium chloride, concentrated sulphuric acid, litmus paper 
(blue), ammonium hydroxide. 

Apparatus. — As in Fig. 41 (or 42). 

I. Preparation. — • (1) Hydrogen chloride. — Put 8 cc. of water 
into a small bottle or an evaporating dish, cautiously add 10 cc. of 
concentrated sulphuric acid, and stir until the two are mixed. While 
this mixture is cooling, weigh 10 gm. of sodium chloride, slip it into 
the flask, and arrange the apparatus as shown in Fig. 41. 

Introduce half of the cold acid mixture into the flask, let it settle 
through the sodium chloride, and then introduce the remaining acid. 
Heat the flask gently with a low flame, as in the preparation of 
chlorine. Hydrogen chloride is evolved, and passes into the bottle 
G, which should be removed when full, as directed under chlorine. 
(A piece of moist blue litmus paper held near the mouth of the bottle 
will show when it is full. Let the gas enter a minute or so after the 


HYDROCHLORIC ACID 65 

first test.) Collect three bottles of the gas, cover each tightly, when 
filled, with a piece of dry filter paper, and set aside for II. 

(2) Hydrochloric acid. — As soon as the third bottle of gas has 
been collected, put in its place a bottle one-fourth full of water. Ad¬ 
just the delivery tube E so that the lower end is a short distance above 
the surface of the water. Continue to heat the flask at intervals, 
and the gas will be absorbed by the water. Shake the bottle occasion¬ 
ally. Meanwhile perform II. 

II. Properties of hydrogen chloride. — a. Insert a blazing joss 
stick once or twice into a bottle of the gas, and observe the result. 
Compare the behavior of hydrogen chloride with that of hydrogen, 
oxygen, carbon dioxide, and chlorine under similar conditions. 

b. Hold a piece of wet filter paper near the mouth (or drop it 
inside) of the same bottle. Observe and describe the result. What 
is the cause? 

c. Invert a bottle of the gas, and stand it in a vessel of water ( e.g . 
the pneumatic trough). Shake the bottle up and down, still keep¬ 
ing its mouth under water. Observe any change inside the bottle. 
What property of the gas does the result illustrate? 

Verify the observation by a simple test applied to the contents 
of the bottle. State the result. 

d. Drop into the remaining bottle of gas a piece of filter paper wet 
with ammonium hydroxide. Describe the result. What is the name 
of the product ? 

e. State other properties of hydrogen chloride observed during 
these experiments, e.g. color, odor, density, behavior with moist lit¬ 
mus paper. 

III. Properties of hydrochloric acid. — Remove the bottle in which 
the hydrogen chloride is being absorbed. 

a. Determine its general properties, e.g. taste (cautiously), ac¬ 
tion with litmus, and with magnesium (using 10 cc. of the hydro¬ 
chloric acid). State the results. 

b. Add to a test tube half full of the hydrochloric acid a few drops 
of silver nitrate solution. Describe the precipitate. What is its 
name? Shake the test tub*e, filter part of the contents, and expose 
the precipitate upon the paper to the sunlight. Describe the change 
in the precipitate which soon occurs. To the remaining contents 
of the test tube add considerable ammonium hydroxide, and shake. 
Describe the result. 

Note. — As soon as III b has been performed, add water to the flask, 
shake well, and pour the contents into a waste jar in the hood. 


66 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 66 — Test for Hydrogen Chloride, Hydrochloric 
Acid, and Chlorides 

a. Recall properties which would serve as a test for (i) hydrogen 
chloride and (2) hydrochloric acid. 

b. Apply the silver nitrate test to a solution of several soluble 
chlorides in separate test tubes (e.g. ammonium chloride, ferric 
chloride, and calcium chloride). State each result. 

Note. — It is customary, though not always necessary, to add nitric 
acid to dissolve compounds other than chlorides which might be formed 
in testing with silver nitrate. 

Experiment 67 — Aqua Regia 

Materials. — Gold leaf, concentrated nitric and hydrochloric acids. 

Touch a small piece of gold leaf with the end of a moist glass rod, 
and wash the gold leaf into a test tube by pouring a few cubic cen¬ 
timeters of concentrated hydrochloric acid down the rod. Warm 
gently. Does the gold dissolve? Wash another piece of gold leaf 
from a clean glass rod into another test tube with concentrated nitric 
acid. Warm as before. Does the gold dissolve ? Pour the contents 
of one tube cautiously into the other. Warm gently, if no change 
occurs. Does the gold dissolve ? 

Answer: 1. What compound of gold is formed by its interaction with 
aqua regia? 

2. Does chlorine water act like aqua regia on gold? 

Experiment 68 — Insoluble Chlorides 

Materials. — Silver, lead, and mercurous nitrate solutions. 

a. Put about 5 cc. of silver nitrate, lead nitrate, and mercurous 
nitrate in separate test tubes, and label each tube. Add 5 cc. of 
dilute hydrochloric acid to each solution, shake, and note the result. 
Describe each precipitate. Name each. * 

b. Shake well, and pour about half of each precipitate into separate 
test tubes. Save the rest of the precipitates for c. 

Fill each of the three test tubes half full of water, and heat to boil¬ 
ing. Note each result. Which chloride dissolves in hot water? 

c. Fill each of the test tubes saved in b with ammonium hydroxide. 
Shake well. Warm gently. Note each result. What is the effect 
of ammonium hydroxide on each chloride? 


ACIDS, BASES, AND SALTS — NEUTRALIZATION 67 


d. Optional. Test unknown solutions for (1) a chloride and (2) lead, 
silver, and mercurous compounds. State each result. 

Answer: 1. In what are these three chlorides insoluble ? 

2. How could the three chlorides be separated from one another? 

3. What is a test for (a) a soluble chloride, ( b) an unknown solution sup¬ 
posed to contain a chloride, (c) a lead compound, ( d ) a silver compound, 
(e) a mercurous compound, (/) lead chloride, ( g) silver chloride, ( h ) mer¬ 
curous chloride? 

4. How can a chloride be distinguished from a sulphate? 

ACIDS, BASES, AND SALTS — NEUTRALIZATION 

(Practical Chemistry, pp. 142-146, §§ 161-167) 

Experiment 69 — General Properties of Acids 

Materials. — Litmus paper (both colors), magnesium ribbon, sodium 
carbonate. 

Fill three test tubes half full of water; add about 5 cc. of dilute 
sulphuric acid to one, of hydrochloric acid to another, and of nitric 
acid to the third. Shake the test tubes thoroughly, and label each. 

a. Dip a clean glass rod into each acid successively and cautiously 
taste it. Describe the taste by a single word. 

b. Dip a clean glass rod into each acid successively and put a drop 
on both kinds of litmus paper. Note the decided change in color. 
The change is characteristic of acids. 

c. Pour out the acids and replace the hydrochloric and sulphuric 
acids with dilute acid from the bottle. Omit the nitric acid. Slip 
a small piece of magnesium ribbon into each test tube. Note the 
results. If no marked chemical action results, warm gently. Test 
the most obvious product by holding a lighted match inside of each 
tube. What gas comes from the hydrochloric and sulphuric acids? 

d. Fill a test tube half full of dilute sulphuric acid, have ready a 
blazing joss stick, add a lump of sodium carbonate to one tube, and 
test the escaping gas. Do the same with the other two acids. What 
is the gas ? 

Experiment 70 — General Properties of Bases 

Materials. — Sodium hydroxide and potassium hydroxide solutions, am¬ 
monium hydroxide, litmus paper (both colors). 

Prepare a very dilute solution of each base as in Exp. 69. 


68 EXPERIMENTS IN PRACTICAL CHEMISTRY 


a. Cautiously taste each liquid by touching to the tip of the 
tongue a rod moistened with each, and describe the result. Compare 
with acids. 

b. Test each solution with litmus paper (both colors). Describe 
the result. Compare with acids. 

c. Rub a little of each undiluted solution from the bottle between 
the fingers, and describe the feeling. 

Experiment 71 — A Property of Many Salts 

- i — .... - ) 


<Z>^- ^ J I / / - ) 

Fig. 44. —Test wires — upper platinum, lower nichrome 

Materials. — Litmus paper (both colors), dilute solutions of chemically 
pure sodium chloride, potassium nitrate, potassium sulphate, barium 
chloride, potassium chlorate, potassium bromide, and strontium 
nitrate. 

a. Test the solutions with litmus paper. Describe the result in 
each case. Compare the litmus reaction of salts with the reaction 
of acids and bases. 

b. Dip a clean glass rod into each solution (except barium chloride) 
successively and cautiously taste it. Do not swallow the liquid. De¬ 
scribe the taste. 


Experiment 72 


Composition of Acids, Bases, and Salts 

I. Acids. — a. Recall or devise an 
experiment to show that hydrogen is 
a constituent of acids, e.g. hydro¬ 
chloric, sulphuric, acetic. 

b. Recall or devise an experiment 
to show that another constituent of 
acids is a non-metallic element or 
group, e.g. Cl, S 0 4 . 

II. Bases. — a. Recall or devise 
an experiment to show that hy¬ 
droxyl (OH) is a constituent of bases. (See Exp. 32 a (3).) 

b. Show by the flame test that a constituent of bases is a metal, 
e.g. sodium, potassium, calcium, barium. Dip a clean test wire 
(Fig. 44) into each solution and hold the end of the wire in the flame 



Fig. 45. — Testing for metals 
by the color of the flame 














ACIDS, BASES, AND SALTS — NEUTRALIZATION 69 

as in Fig. 45. The flame is colored yellow by sodium, pale violet 
by potassium, red by calcium, and green by barium. Concentrated 
calcium hydroxide, or the powdered substance, should be used. 

III. Salts. — a. Recall or devise experiments to show that a con¬ 
stituent of salts is a metal, e.g. sodium, potassium, calcium, barium, 
silver, lead, mercury (mercurous). 

b. As in a, also a non-metallic element or group of elements — 
the same as in I b. 

Answer: 1. What is a constituent common to acids ? To bases? 

2. What class of elements, single or in groups, is a constituent of acids? 
Of bases ? 

3. What classes of elements, single or in groups, are constituents of 
salts ? 


Experiment 73 — Testing for Acids and Bases 

Materials. — Lemon juice, vinegar, sweet and sour milk, wood ashes, 
faucet water, cream of tartar, the juice of any ripe fruit and any un¬ 
ripe fruit, household ammonia, potash, limewater, pickles, jelly, grape 
juice, lye, “unknowns.” 

Apply the litmus test to the substances enumerated above. Make 
a solution of each of the solids before testing. Tabulate the results 
under the terms, Acid and Basic. 

Experiment 74 — Neutralization 

Materials. — Sodium hydroxide (solid), blue litmus paper. 

Dissolve a small piece of sodium hydroxide in an evaporating dish 
one-third full of water. Add a little dilute hydrochloric acid, and 
stir thoroughly; continue to add the acid, until a drop of the well- 
mixed solution taken from the dish by a clean glass rod just reddens 
blue litmus paper. If the dish becomes too full, pour out some of 
the solution. 

Evaporate the solution to dryness by heating the dish on a gauze- 
covered ring. Heat until the yellow color (due to the slight excess 
of hydrochloric acid added) disappears, then moisten the whole residue 
carefully with a little warm water, and heat again to evaporate the 
last traces of acid; add and evaporate two portions of water. 

Test small portions of the residue. (1) Apply the litmus test. 
Has the residue acid, basic, or neutral properties? (2) Taste a 
little. Is it an acid, base, or salt ? (3) Dissolve some in water and 


70 EXPERIMENTS IN PRACTICAL CHEMISTRY 


test the solution for a chloride. State the result. (4) Test for 
sodium by heating a little on a test wire in the flame. State the 
result. What is the residue? Write the equation for the re¬ 
action. 


Experiment 75 — Neutralization by Titration 




Object. — To find the number of grams of the 
compound HC 1 in 1 cc. of a solution of hydro¬ 
chloric acid (i.e. HC 1 dissolved in water) by neu¬ 
tralizing the acid with a solution of sodium hy¬ 
droxide of known concentration. 

Materials. — Phenol-phthalein solution, and so¬ 
lutions of hydrochloric acid and sodium hydrox¬ 
ide (the latter of known concentration and ob¬ 
tained from the Teacher). 

Apparatus. — Burettes, beakers, and glass rod as in 
Fig. 46, waste beaker. 

Copy the form of Record given below in the 
notebook and enter each volume as soon as the 
reading is made. 

Fill each burette (or start with each full) — 
one with the acid solution and one with the 
base solution (Fig. 46). Be sure the tip of 
the burette is free from air bubbles. Place the 
waste beaker under each burette in turn and 
allow the solution to run out slowly until the 
bottom of the meniscus rests on the o line when the eye is on a 
level with the same line. (See Fig. 47.) 



Fig. 46. — Burettes 
for accurate ex¬ 
periments in neu¬ 
tralization 


Set the waste beaker aside. 

Put a clean beaker under the base bu¬ 
rette and let exactly 15 cc. run into the 
beaker; enter in I in the Record. Remove 
the beaker, add 2 or 3 drops of phenol- 
phthalein solution, put the beaker under 
the acid burette, and let the acid solution 
run in slowly, stirring constantly with the 
clean rod until the red color just disappears 
and the solution becomes colorless. Read 
the exact volume of acid solution added 
and enter in I. 




12- 




Fig. 47. — Meniscus 
(correct reading along 
line I) 




















ACIDS, BASES, AND SALTS — NEUTRALIZATION 71 


Record 


I. NaOH sol. o — 15 = 15 
HC 1 sol. o - = 

II. NaOH sol. 15 — 30 = 15 
HC1 sol. 

III. NaOH sol. 30 — 45 = 15 
HC 1 sol. - 

.*. 1 cc. NaOH sol. = 


1 cc. NaOH sol. = cc. HC 1 sol. 

1 cc. NaOH sol. = cc. HC 1 sol. 

1 cc. NaOH sol. = cc. HC 1 sol. 

cc. HCl sol. (average) 


Pour the solution out of this beaker, wash the beaker, and proceed, 
as before, with a second 15 cc. of NaOH solution. Enter in II. 

Wash the beaker and proceed with a third 15 cc. of NaOH solution. 
Enter in III. 

Calculation. — Our problem is to calculate the number of grams 
of HCl in 1 cc. of the solution of hydrochloric acid used in this ex¬ 
periment. 

(a) First write the equation for the reaction, thus : — 

HCl + NaOH = NaCl + H 2 0 
36.5 40 58.5 18 

This equation means that 36.5 gm. of HCl are needed to neutralize 
40 gm. of NaOH. 

(b) Next find (from I, II, III, above) the average number of cubic 
centimeters of hydrochloric acid solution which would be neutralized 
by 1 cc. of sodium hydroxide solution. For example, suppose 1.5 cc. 
HCl sol. = 1 cc. NaOH sol. (Your result, of course, may be differ¬ 
ent from this value.) 

(c) Learn from the Teacher the concentration of the sodium hy¬ 
droxide solution. For example, suppose 1 cc. of sodium hydroxide 
solution contains 0.00641 gm. of NaOH. 

( d ) Now from the equation in ( a ) we see that 40 gm. of NaOH re¬ 
quire 36.5 gm. of HCl. Then the number of grams of HCl required 
by 0.00641 gm. of NaOH would be found by the proportion 

40 : 36.5 :: 0.00641 : x x = o 00585 

(Your result depends on the concentration of your NaOH solution.) 
But 0.00585 gm. of HCl would be dissolved in 1.5 cc. of hydrochloric 
acid (according to our supposition in ( b )). Therefore, to find the 
number of grams of HCl that would be dissolved in 1 cc. of the acid 
solution, we divide 0.00585 by 1.5, i.e. 0.00585 -f- 1.5 = 0.0039. 
Ans. 0.0039 g m - HCl in 1 cc. 


72 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 76 — Preparation of a Salt by Various Methods 

Materials. — Calcium, calcium oxide, carbonate, and chloride, silver 
nitrate solution. 

a. Acid and a metal. — Put a small piece of calcium in an evapo¬ 
rating dish, add a little dilute hydrochloric acid, stand the dish on a 
gauze-covered ring, and heat gently in the hood until the calcium 
disappears, adding more acid if necessary. Then evaporate the 
solution to dryness; heat gently toward the end to prevent spatter¬ 
ing. Moisten the residue with water, and evaporate again to dry¬ 
ness. Heat the residue until no more fumes of hydrochloric acid are 
evolved. Let the dish cool, and loosen the solid with a glass rod. 

Test small portions of the residue for (i) calcium (flame test), 
and (2) a chloride. State the result. 

b. Acid and an oxide. — Proceed as in a, using hydrochloric acid 
and a small piece of calcium oxide. Test the final residue as in a. 
State the result. 

c. Acid and a salt. — Proceed as in a, using hydrochloric acid and 
a small piece of calcium carbonate. Test the final residue (as in a). 
State the result. 

d. Two salts. — Add silver nitrate solution to calcium chloride 
solution, and describe the result. 

Required Exercises. — 1. What is the name and formula of the resi¬ 
due in each part of this experiment? Write the equation for each re¬ 
action. 

2. Suggest a simple experiment to verify the answer in 1. 

3. Suggest experiments to prove that the residue is neither an acid nor 
a base. 

e. Acid and base. —Recall an experiment in which a salt was 
formed by the interaction of an acid and a base. Name all the com¬ 
pounds involved in the reaction. Write the equation. 


AMMONIA — AMMONIUM COMPOUNDS 

(Practical Chemistry, pp. 148-157, §§ 168-181) 

Experiment 77 —Ammonia (Gas) and Ammonium Hydroxide 

Materials. — Lime (calcium oxide), ammonium chloride, concentrated 
hydrochloric acid. 

Apparatus. — As in Fig. 48. The test tube A is provided with a one-hole 


AMMONIA — AMMONIUM COMPOUNDS 


73 


rubber stopper to which is fitted a glass tube B which reaches well up 
into the bottle C, 3 bottles, pneumatic trough filled as usual. Optional 
forms of apparatus (as in Fig. 49) may be used. 

Caution. — Do not inhale ammonia (gas). 

Perform this experiment in the hood. 

Weigh 10 gm. of lime and 10 gm. of 
ammonium chloride separately, and mix 
them thoroughly on. a piece of paper. Slip 
the mixture into A , and add a little water, 
thereby transforming the calcium oxide into 
calcium hydroxide. Mix well. Quickly insert 
the stopper with its tube, and clamp A as 
in Fig. 48. Stand the bottle C over the 
tube B. 

Heat A gently with a low flame. (Begin 
to heat the test tube near the closed end 
and slowly work forward to the delivery 
tube.) Ammonia (gas) will pass up into the 
bottle, which should be removed, when full, and covered tightly 

with a glass plate or filter paper. A 
piece of moist red litmus paper held 
near the mouth will show (by change 
in color) when the bottle is full. Do 
not smell at the mouth of the bottle. 
Collect two bottles of the gas. 

a. Test the gas in one bottle or test 
tube with a blazing joss stick. Ob¬ 
serve the result. Compare with the 
behavior of oxygen, carbon dioxide, 
hydrogen, and hydrogen chloride 
under similar circumstances. 

b. Invert the same bottle in the 
pneumatic trough, and shake it vig¬ 
orously, taking care to keep the 
mouth under water. Observe the 
change inside the bottle. What prop¬ 
erty of the gas is revealed? Is it a 

marked property? Test the contents of the bottle with litmus paper 
(both colors), and state the result. 

c. Pour a few drops of concentrated hydrochloric acid into an 
empty, warm, dry bottle. Rotate the bottle until the inside is well 
moistened with the acid. Cover it with a glass plate, invert it, and 



for preparing am¬ 
monia (gas) 



Fig. 48. — Apparatus 
for preparing am¬ 
monia 



























74 EXPERIMENTS IN PRACTICAL CHEMISTRY 


stand it upon a covered bottle of ammonia (gas). Remove both 
plates at once, and hold the bottles together by grasping them firmly 
about their necks. Observe the result. Describe the result, giving 
the evidence of the chemical action. What is the white substance? 

d. State other properties of ammonia (gas) you have observed in 
this experiment, e.g. color, odor, density, and behavior with moist 
litmus paper. 

Experiment 78 —Ammonia (Gas) from Various Substances 

Materials. — Gelatin, soda-lime, litmus paper, concentrated hydrochloric 
acid, substances enumerated in b, ammonium sulphate, ammonium 
nitrate, sodium hydroxide solution, calcium cyanamide (for f), am- 
moniacal liquor (for g). 

a. Mix a little gelatin and soda-lime on a piece of paper, slip the 
mixture into a test tube, attach a test tube holder, heat, and test the 
escaping gas with moist red litmus paper, or by a glass rod moistened 
with concentrated hydrochloric acid. State the result. 

b. Repeat a, using soda-lime with hair, feather, leather scraps, or 
pieces of horn. Observe and state the results. 

c. Dissolve a little ammonium chloride in water, add a little sodium 
hydroxide solution, warm gently, and test (cautiously) the liberated 
gas by its odor. What is the gas ? 

d. Repeat c, using ammonium sulphate and sodium hydroxide 
solution. State the result. 

e. Proceed as in d, using ammonium nitrate. Test (by the odor) 
the gaseous product, and state the result. 

f. Put about 5 gm. of calcium cyanamide in a test tube, add io cc. 
of water, shake, boil, and test for ammonia. State the result. 

g. Optional. Add powdered calcium oxide (lime) to a test tube 
half full of ammoniacal liquor, warm gently, and test the escaping 
gas for ammonia. State the result. 

Experiment 79 — Properties of Ammonium Salts 

Materials. — Ammonium chloride, sodium hydroxide, sand, ammonium 
nitrate, ammonium carbonate. 

a. Examine ammonium chloride and state its characteristic prop¬ 
erties. 

b. Add a few grams of ammonium chloride to a test tube half full 
of water, shake well, and observe the result. Does ammonium 
chloride dissolve easily in water? Add a little more of the salt, shake, 


NITRIC ACID — NITRATES — NITROGEN OXIDES 75 


and note how the dissolving affects the temperature of the solvent. 
Save the solution for c. 

c. Add a small piece of sodium hydroxide to the solution from b, 
warm gently, and very cautiously observe the odor of the gaseous 
product. What is the gas? Explain its formation. 

d. Put a little crude ammonium chloride (or a mixture of ammo¬ 
nium chloride and sand) in a clean, dry test tube, heat the closed end 
gently, and observe the result. What is the white deposit? Heat 
intensely. Is there a residue? If so, compare it with the white 
deposit. What general name is given to this process? To the prod¬ 
uct? 

e. Add a little ammonium nitrate to sodium hydroxide solution 
in a test tube, warm gently, and cautiously note the gaseous product. 
What is it ? Moisten a glass rod with concentrated nitric acid and 
hold it at the mouth of the test tube (after warming again, if neces¬ 
sary). Describe the result. What is the product? 

f. Smell of a lump of ammonium carbonate. To what substance 
is the odor due? Moisten with water and smell again. What is 
the product ? 

Answer: 1. What is the test for ammonium compounds? 

2 . What is the equation for the reaction in c? For the two reactions 
in e? 

Experiment 80 — Testing Salts (Review) 

Materials. — Chlorides, sulphates, carbonates, and nitrates of sodium, 
potassium, calcium, barium, and ammonium; nitrates of silver, lead, 
and mercury; dilute hydrochloric acid. 

Obtain several “ unknowns ” from the substances enumerated 
above and test a separate portion of each for (a) the metal part, i.e. 
sodium, potassium, calcium, barium, silver, lead, ammonium, and 
(b) the non-metal part, i.e. a chloride, a sulphate, and a carbonate. 
State each result. Give the name and formula of each salt. 

NITRIC ACID — NITRATES — NITROGEN OXIDES 

(Practical Chemistry, pp. 159-170, §§ 182-197) 

Experiment 81 — Nitric Acid 

Materials. — Sodium nitrate, concentrated sulphuric acid, quill tooth¬ 
pick, copper wire, zinc, magnesium ribbon. 

Apparatus. — Glass stoppered retort, etc., as in Fig. 50. 


76 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Caution. — Concentrated nitric acid and sulphuric acid are very 
corrosive. Do not spill them on the flesh or the clothing. 

Note. —I may be omitted and II done with concentrated nitric acid 
from the laboratory bottle. 

I. Preparation. — Weigh 20 gm. of sodium nitrate and slip it into 
the retort through the tubulure. Fill the bottle nearly full of water. 

Put a large empty test tube 
into the bottle, insert the neck 
of the retort into the test tube, 
and arrange the apparatus as 
shown in Fig. 50. Stand a 
funnel in the tubulure of the 
retort so that the end is well 
inside the bulb, and pour 20 cc. 
of concentrated sulphuric acid 
through the funnel. Remove 
the funnel and insert the stop¬ 
per of the retort tightly. 

Heat the retort gently as 
long as any nitric acid runs 
down the neck into the test 
tube. Then unclamp the 
retort and remove the test 
tube carefully, taking care not to get any nitric acid on the hands. 

Note. — Allow the contents of the retort to cool, add a little water, boil 
until the solid in the bulb is reduced to a small bulk or dissolved, and pour 
it into a waste jar in the hood. 

II. Properties. — a. Observe the color of the concentrated nitric 
acid prepared in I. Compare it with the concentrated nitric acid in 
several bottles in the laboratory and with the typical specimen of 
concentrated nitric acid placed upon the side shelf by the Teacher. 
State the result. 

b. Hold a piece of wet filter paper at the mouth of the test tube 
of concentrated nitric acid. Observe and state the result. 

c. Repeat b, using a piece of filter paper moistened with ammo¬ 
nium hydroxide. What is the name of the product? 

d. Pour 5 cc. of concentrated nitric acid very carefully into a test 
tube, drop in a piece of a quill toothpick, and observe any change in 
the color of the quill. Heat very gently, and observe the effect on 
the quill. State the final result. 



Fig. 50. —Apparatus for preparing nitric 
acid in the laboratory 














NITRIC ACID — NITRATES — NITROGEN OXIDES 7 7 


e. Put about 1 gm. of sulphur in a test tube, add a little water 
and then very carefully 5 cc. of concentrated nitric acid. Attach 
the test tube holder, and boil cautiously — in the hood — for a few 
minutes. Add 10 to 15 cc. of water, filter the solution, if it is not 
clear, and test the filtrate for a sulphate by adding barium chloride 
solution. State the result. Explain it. 

f. Stand three test tubes in the test tube rack, put a piece of zinc 
into one, copper into another, and magnesium ribbon (rolled into a 
ball) into the third. Add a little concentrated nitric acid to each 
test tube. Observe the result. Test the gaseous product for hydro¬ 
gen, and state the result. 

Required Exercises. — 1. What property of nitric acid was shown by 
b? Byd? Bye? 

2. How does the action in b and c compare with that of hydrochloric, 
acid under similar circumstances? 

3. Apply Exercise 2 to f. (If in doubt, try the experiment.) 

Experiment 82 — Properties of Nitrates 

Materials. — Copper nitrate, lead nitrate, potassium nitrate, charcoal. 

a. Put a little copper nitrate in a test tube, attach the holder, heat 
gently, and observe the result, especially the color of the gaseous 
product and of the final solid product. Test the gaseous product 
for oxygen. State the result. 

Devise an experiment to determine the qualitative composition of 
the solid product; consult the Teacher before proceeding. 

b. Pulverize a little lead nitrate and proceed with it as in a. State 
the results. 

c. Proceed as in Exp. 9 a. 


Experiment 83 — Interaction of Nitric Acid and Metals 

Materials. — Zinc, copper, tin, iron, concentrated nitric acid. 

Stand four test tubes in the test tube rack. Slip into one a few 
pieces of zinc, into another a small piece of tin, into the third a small 
quantity of copper borings, and into the fourth a small quantity of 
clean iron filings. Add to each test tube in succession enough con¬ 
centrated nitric acid to cover the metal. Warm slightly, if there is 
no action. Observe and describe the changes, particularly (1) the 
vigor of the action, (2) the properties of the solid products, espe¬ 
cially color and solubility, and (3) the properties of the gaseous prod- 


78 EXPERIMENTS IN PRACTICAL CHEMISTRY 


ucts. Name the solid product and the gaseous product of the re¬ 
action in each case. 

Experiment 84 — Test for Nitric Acid and Nitrates 

Materials. — Ferrous sulphate, sodium nitrate. 

a. To io cc. of water add i or 2 cc. of concentrated nitric acid and 
shake. Prepare a ferrous sulphate solution by dissolving a clean 
crystal in 10 cc. of cold water. 

Pour this solution into the nitric acid. Mix well. Incline the 
test tube and pour about 5 cc. of concentrated sulphuric acid down 
the inside of the tube. The sulphuric acid will sink through the other 
liquid. At the surface where the two solutions meet, a brown or 
black layer will appear (Fig. 51). 

b. Proceed as in a, using a concentrated solution of sodium nitrate 
instead of nitric acid. Record the result. 


Experiment 85 — Nitric Oxide and Nitrogen Dioxide 


Materials. — Copper (borings or fine pieces of sheet metal), concentrated 
nitric acid, piece of copper wire (15 cm. or 6 in. long). 

Put 10 gm. of copper in the bottle, and arrange the apparatus to 
collect the gas over water (Fig. 52). Fill three 
bottles with water, and invert one of them in the 
trough. Have the others ready. 

Dilute 25 cc. of concentrated nitric acid with an 
equal volume of water, and introduce just enough 
of this dilute acid through the dropping tube to 
cause gentle chemical action. If the action is too 
vigorous, add water through the dropping tube; 
if too weak, add a little of the dilute nitric acid. 
Fig. 51. — Test Collect three bottles of the gas, which is nitric 
for nitric acid oxide, and cover them with glass plates, 
and nitrates a. Observe the general properties of nitric 

oxide while covered. 

b. Uncover a bottle. Observe the result. Is the brown gas, 
which is formed, identical in color with the one observed in the gen¬ 
erator at, the beginning of the experiment? What is the brown gas? 

c. Uncover a bottle, let the brown gas form, then pour in about 
25 cc. of water, cover with the hand and shake vigorously, still keep¬ 
ing the bottle covered. Does the brown gas disappear? 





NITRIC ACID — NITRATES — NITROGEN OXIDES 79 


d. With the third bottle, determine whether the gases will burn 
or support combustion. A convenient flame is a burning match 



Fig. 52. — Apparatus for preparing 
nitric oxide 


fastened to a copper wire. 
Uncover a bottle and plunge 
the lighted match quickly to 
the bottom of the bottle and 
immediately replace the glass 
plate. Observe the result. 
Remove the glass plate and 
observe the result. 

Required Exercises. — 1. Sum¬ 
marize the properties of nitric 
oxide. Of nitrogen dioxide. 

2. What is the general chemical 
relation of the two gases to each 
other? To the air? 

3. Why cannot nitrogen dioxide 
be collected over water? 


Experiment 86 — Preparation and Properties of Nitrous Oxide 


Materials. — Ammonium nitrate, wad of iron thread, copper wire, sul¬ 
phur, joss stick. 

Put 10 gm. of ammonium nitrate 
in the flask A . Construct and 

arrange the apparatus as shown in 
Fig. 53. The large test tube B 
remains empty. The end of H rests 
on the bottom of the pneumatic 

trough, which is filled as usual. Be 
sure the apparatus does not leak. 

I. Preparation. — Heat the flask 
gently with a low 
flame, and read¬ 
just the appara¬ 
tus if it leaks. 

The ammonium 
nitrate melts at 

first and soon ap¬ 
pears to boil, owing p IG ^ — Apparatus for preparing nitrous oxide 

to the decomposi¬ 
tion of the salt and escape of nitrous oxide. Regulate the heat so 












































8 o EXPERIMENTS IN PRACTICAL CHEMISTRY 


that the evolution of the nitrous oxide is slow. Notice the liquid 
which collects in B. Collect three bottles of nitrous oxide, cov¬ 
ering each with a piece of filter paper as soon as removed from, 
the trough. When the last bottle has been collected and covered, 
remove the end of the delivery tube from the trough. 

II. Properties. — a. Allow a bottle to remain uncovered for a few 
seconds. How does nitrous oxide differ from nitric oxide ? Nitrogen 
dioxide ? 

b. Thrust a glowing joss stick into the same bottle of gas. Ob¬ 
serve the result. Is the gas combustible ? Does it support combus¬ 
tion? 

c. Put a piece of sulphur in a deflagrating spoon, light it, and lower 
the burning sulphur at once into another bottle of gas. Observe the 
result. 

d. Twist one end of the copper wire around a wad of iron thread. 
Heat the edge of the wad an instant in the flame and then lower it 
quickly into a bottle of the gas. Observe the result. Recall a simi¬ 
lar experiment with oxygen. Compare the two results. 

Required Exercises. — i. Summarize the essential properties of 
nitrous oxide. 

2. What is the other product (seen in B) of the chemical change in this 
experiment ? 

3. How could you distinguish ammonium nitrate from other nitrates? 

4. How could you distinguish nitrous oxide from ( a ) the other oxides 
of nitrogen, ( b ) air, (c) oxygen, ( d) hydrogen, ( e ) nitrogen, (/) carbon 
dioxide ? 


MOLECULAR WEIGHTS 

(Practical Chemistry, pp. 171-180, §§ 198-208) 

Experiment 87 — Weight of 22.4 Liters of Carbon Dioxide 

Object. — To find the volume of carbon dioxide liberated from a weighed 
amount of calcium carbonate and to calculate the weight of 22.4 1. of 
this gas. 

Materials. — Crystallized calcium carbonate, concentrated hydrochloric 
acid. 

Apparatus. — As in Fig. 54, glass plug for stopper of A. A is a 125 cc. 
Erlenmeyer flask in which the carbon dioxide is generated. The large 
bottles C and E are dry and empty. G is a 750 cc. bottle filled with 
water and inverted in the pneumatic trough as usual. 


MOLECULAR WEIGHTS 


81 


Copy the form of Record as given below in your notebook and 
enter each item as soon as the weighing or measuring is made. 

Construct and ar¬ 
range the apparatus 
as in Fig. 54. Put 20 
cc. of concentrated 
hydrochloric acid and 
5 cc. of water in A, 
mix well, add a small 
piece of unweighed cal¬ 
cium carbonate, insert 
the stopper loosely, and 
let the flask remain 
undisturbed until the 
calcium carbonate dis¬ 
appears ; the object of this is to fill A with carbon dioxide before 
weighing (since it is full of the gas at the end). 

Meanwhile weigh accurately on the balance 2.5 to 3 gm. of calcium 
carbonate. (See Introduction, § 8, for instructions about weighing.) 
Enter the weight as ( b ) below. When the evolution of gas stops in 
A insert a glass plug in the hole of the stopper and weigh the whole 
on the balance. Record the weight as (a) below. Remove and 
preserve the plug. 



Fig. 54. 


- Apparatus for finding the weight of 
22.4 liters of carbon dioxide 


Record 


Thermometer (/).... 0 Barometer ( P ') . . mm. 

(a) Weight of flask, stopper, plug, and acid. gm. 

(b) Weight of calcium carbonate. gm. 

(c) Weight of flask, stopper, plug, etc. — before action . . gm. 

(1 d ) Weight of flask, stopper, plug, etc. — after action --gm. 

(e) Weight of carbon dioxide ( (c) — (d) ). gm. 

(/) Volume of carbon dioxide (observed). cc. 

( g ) Volume of carbon dioxide (corrected). cc. 

(h) Weight of a liter of carbon dioxide . gm. 

( i ) Weight of 22.4 liters of carbon dioxide. gm. 


Carefully push A with its stopper upon the tube B, remove the 
flask, hold it near the stopper, slip in the weighed calcium carbonate 
and instantly push the flask firmly upon the stopper. The carbon 
dioxide soon forces air into G. If no bubbles arise in G, examine the 
apparatus for a leak and quickly readjust, if necessary. 

Let the operation continue until the gas ceases to rise in G. Then 



























82 EXPERIMENTS IN PRACTICAL CHEMISTRY 


carefully joggle G to dislodge any bubbles which may be underneath 
the support. Slide the bottle from the support down upon the bot¬ 
tom of the trough. Add water to the trough, if the level is below 
the level inside the bottle; if unnecessary, raise the bottle until the 
water is at the same level inside and outside. Slip two pieces of 
filter paper beneath the bottle, cover the mouth firmly, invert and 
remove, and stand it right side up on the table. Stand a thermome¬ 
ter in the bottle, and read and record the temperature (t) after a few 
moments. Also read and record the barometer (P'). 

Fill a large graduate (preferably 1000 cc.) with water to the mark 
and pour water carefully from the graduate into G until full. Read 
the exact volume of the water added to G and record as (/); this is 
the volume of carbon dioxide liberated. Correct it for temperature, 
pressure, and aqueous tension by the method given in Exp. 24. Enter 
the corrected volume as (g). 

Weigh A with its contents, stopper, and plug, and enter the weight 
as ( d ). 

From the weight of carbon dioxide ( (c) — (d) ) and the corrected 
volume (g) calculate the weight of a liter, and record as (h) above. 
Multiply this weight {h) by 22.4 and record as (t). 

Answer: 1. What is the exact weight of a liter of carbon dioxide? What 
weight did you obtain? What is the class average? 

2. What is the weight of 22.4 liters of carbon dioxide calculated from 
the class average of the weight of one liter? 

3. What is the weight of 22.4 liters of oxygen calculated from the class 
average of Exp. 24? 


EQUIVALENT WEIGHTS 

(Practical Chemistry, pp. 182-190, §§ 209-216) 

Experiment 88 — Equivalent of Zinc (to Hydrogen) 

Object. — To find the number of grams of zinc chemically equivalent to 
one gram of hydrogen. 

Apparatus. — As in Fig. 55, pneumatic trough (not zinc), thermometer, 
barometer. 

Copy the form of Record in the notebook and enter each weight 
or volume as soon as the weighing or measuring is made. 

Construct and arrange the apparatus (Fig. 55) to collect a gas 
over water, and have it inspected by the Teacher. 


EQUIVALENT WEIGHTS 


83 

Weigh from 0.45 to 0.5 gm. of zinc on the balance. Take a single 
piece and weigh it exactly. Enter in the Record as Zn. 

Record 


Weight of zinc taken {Zn) . 

Observed volume of hydrogen (F') . . 

Temperature (t) . 

Pressure (P') . 

Vapor pressure ( a ). 

Corrected volume of hydrogen (F) . . 

Weight of corrected volume of hydrogen (W) 

Equivalent of zinc (£). 

Put the weighed zinc into the bottle A. Fill the bottle with water 
and insert the stopper with all 
its tubes. Next fill the re¬ 
mainder of the apparatus with 
water by first filling the cup 
with water and then admitting 
it repeatedly until all air is 
forced out of the bottle and 
tubes; take care never to let 
the water in B fall below the 
lower opening of the cup. 

Note that the inner end of the 
tube C does not extend below 
the stopper. 

Fill a 250 cc. bottle with 
water and invert it upon the Fig ' 55 -- Apparatus for finding the 
support in the trough (a sheet equivalent of zinc 

zinc trough must not be used). 

Put the end of the delivery tube under the support and ask for a 
final inspection. Heat about 50 cc. of dilute sulphuric acid in a 
test tube. Fill the cup and introduce the hot acid in separate por¬ 
tions slowly into the bottle A, taking the same care as before. 
The liberated hydrogen will slowly accumulate in the receiving 
bottle. 

Let the action continue until the zinc is used up. Then force over 
into the collecting bottle all gas in the apparatus by admitting 
water carefully as before. Lay a piece of dry filter paper upon 
the bottom of the bottle, grasp the bottle firmly, carefully joggle it 
to dislodge any gas bubbles which may be underneath the support, 



gm. 

cc. 

o 

mm. 

mm. 

cc. 

gm. 

gm. 



























84 EXPERIMENTS IN PRACTICAL CHEMISTRY 

slide the bottle from the support, and lower it into the water until 
the water is at the same level inside and outside the bottle; then 
slip two pieces of filter paper beneath the bottle, cover the mouth 
firmly, lift the bottle from the trough and stand it, right side up, 
upon the table. Stand a thermometer in the trough. 

Fill a 250 cc. graduate exactly to the mark with water, remove the 
paper cover from the bottle, and very carefully fill the bottle with 
water from the graduate; read and enter (as V') the exact volume 
of water added; this is the volume of hydrogen liberated. Read 
the thermometer while the bulb is in the water, and enter as t. Read 
the barometer, and enter as P'. Find the vapor pressure correspond¬ 
ing to the observed temperature (see Appendix, § 4), and enter as a. 

Correct the observed volume (F') of hydrogen for temperature, 
pressure, and vapor pressure, and enter as F. Since 1000 cc. of 
dry hydrogen weigh 0.09 gm., the weight ( W ) of the corrected volume 
(F) is found by 1000: F :: 0.09 : IF. And the weight of zinc equiva¬ 
lent ( E ) to one gram of hydrogen is found by W : Zn :: 1 : E. Enter 
the equivalent of zinc as E. Submit the result to the Teacher before 
taking the apparatus apart. 

Required Exercises. — 1. Calculate the atomic weight of zinc by 
multiplying the equivalent weight (found in this experiment) by 2. 

2. Compare this calculated atomic weight with the approximate atomic 
weight. 

3. Calculate, as in Exercise 1, from the class average. 

4. Compare the number obtained in 3, as in Exercise 2. 

Experiment 89 — Equivalent of Magnesium (to Hydrogen) 

Object. — To find the number of grams of magnesium equivalent to 1 gm. 
of hydrogen. 

Materials. — Magnesium ribbon, concentrated hydrochloric acid. 
Apparatus. — A 100 cc. tube, pneumatic trough (not zinc), thermometer, 
barometer, tall jar ( e.g . 1000 cc. graduate). 

Prepare a form of Record like that in Exp. 88 and enter the items, 
when available, in the proper place. 

Weigh accurately from 0.06 to 0.07 gm. of magnesium ribbon, 
preferably in a single piece. Enter the exact weight as Mg. Have 
the trough (not zinc) half full of water. Pour 10 cc. of concentrated 
hydrochloric acid into the 100 cc. tube and fill the tube completely 
with cold water. Put the magnesium into the water in the tube, 
cover the end of the tube with the thumb or finger, invert and stand 


EQUIVALENT WEIGHTS 


85 


it in the trough, but keep the end loosely closed to prevent the mag¬ 
nesium from slipping out. As the acid sinks through the water and 
reaches the magnesium, action begins vigorously. Hydrogen rises 
rapidly in the tube and usually carries the magnesium with it. Watch 
the operation, and shake the tube to prevent the magnesium from 
sticking to the inside. If a piece of magnesium should stick to 
the inside of the tube, close the end of the tube tightly, lift it from 
the water, incline it enough to let the liquid run down and loosen the 
magnesium, and then quickly put the end of the tube beneath the 
water. 

When all the magnesium has disappeared, close the end of the 
tube, remove the tube to a tall jar of water, and let it stand five or 
more minutes; then, by a clamp (without touching the tube with the 
hands) adjust the height so that the water levels are the same inside 
and outside of the tube. Read the volume of hydrogen, and enter 
as the observed volume (F')« Read the barometer and the ther¬ 
mometer (keeping the bulb in the water). 

Correct the observed volume (F 7 ) for temperature, pressure, and 
vapor pressure, and enter as the corrected volume ( V '). Find the 
weight (IF) of this volume (F) of hydrogen. Calculate the equiva¬ 
lent of magnesium to hydrogen, as in Exp. 88. Enter the equiva¬ 
lent of magnesium as E. 

Required Exercises. — As in Exp. 88. 

Experiment 90 — Equivalent of Aluminium (to Hydrogen) 

Proceed as in Exp. 88. Use about 0.17 gm. of aluminium (taking 
care to weigh exactly the amount used). Use hot concentrated hy¬ 
drochloric acid instead of dilute sulphuric acid. Record and cal¬ 
culate as in Exp. 88. 

Required Exercises. — As in Exp. 88. 

Note. — The multiplier in Exercise 1 is 3. 

Experiment 91 — Equivalent of Calcium (to Hydrogen) 

Proceed as in Exp. 89. Use about 0.11 gm. of calcium. Record 
and calculate as in Exp. 89. 

Required Exercises. — As in Exp. 88. 

Experiment 92 — Equivalent of Zinc (to Oxygen) 

Object. — To prepare zinc oxide from a weighed amount of zinc and to 
find the relative weights of zinc and oxygen. 


86 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Apparatus. — Evaporating dish fitted with a glass cover, pointed glass 
tube, water bath. 

Copy the form of Record given below in your notebook, and 
enter each weight as soon as the weighing is made. 

Clean and dry an evaporating dish. Weigh it on the balance 
accurately. Put about i gm. of zinc in it, weigh again, and enter 
the exact weight. 

Record 


Weight of dish and zinc. gm. 

Weight of dish. gm. 

Weight of zinc. gm. 

Weight of dish and zinc oxide I gm., II gm., Ill gm. 

Weight of dish. gm. 

Weight of zinc oxide. gm. 

Weight of zinc. gm. 

Weight of oxygen. gm. 


Stand it on a crucible block, add 5 cc. of water, cover the dish with 
a glass cover (preferably a watch glass — convex side down), and 
add concentrated nitric acid, a little at a time, by letting the acid 
run into the dish from a pointed tube held in the opening between 
the cover and the lip of the dish. Add acid at intervals until the 
zinc disappears. Then remove the glass cover, hold it edgewise over 
the dish, and rinse off the drops into the dish by pouring a little water 
upon the upper part of the cover. 

Stand the dish on a water bath and let the liquid evaporate (with¬ 
out the glass cover). When only a small amount of sirupy liquid is 
left, transfer the dish from the water bath to a crucible block, carry 
it to the hood, stand it on a gauze-covered ring, and heat very gently 
with a low flame. Hold the burner in the hand, and regulate the heat 
to prevent spattering. Continue to heat as the mass thickens and 
gives off red fumes; as soon as the mass becomes perfectly dry, heat 
strongly for about five minutes. Cool, weigh, and enter the weight 
as I. Heat again intensely for five minutes, cool, weigh, and enter 
as II. If the weights are not the same, submit the result to the 
Teacher. A third heating and weighing may be necessary. 

The zinc was changed to zinc nitrate by the acid, and the nitrate 
to zinc oxide by heating. The equivalent weight of oxygen is 8. 
Calculate the equivalent weight of zinc to oxygen. Submit the re¬ 
sult to the Teacher before removing the zinc oxide from the dish. 

Required Exercises. — As in Exp. 88. 













IONS AND IONIZATION 


*7 


Experiment 93 — Equivalent of Zinc (to Chlorine) 

Object. — To prepare zinc chloride from a weighed amount of zinc and 
to find the relative weights of zinc and chlorine. 

Apparatus. — As in Exp. 92, desiccator (optional). 

Prepare a form of record like that in Exp. 92, substituting chloride 
for oxide and chlorine for oxygen. 

Weigh a clean, dry porcelain dish accurately. Add from 1.5 to 
2 gm. of zinc, and weigh exactly. Record 
each weight. Introduce concentrated hydro¬ 
chloric acid (instead of nitric acid) into the 
covered dish as in Exp. 92. Evaporate on 
the water bath until nothing escapes from 
the dish. Then transfer the dish to a gauze- 
covered ring and heat gently with a low flame 
to remove the last portion of water. Zinc 
chloride is volatile at a low temperature. 

Hence, it must be heated gently. Remove 
the flame as soon as fumes begin to appear. 

Pass the flame over the surface occasionally 
to assist the removal of the last traces of 
water. 

When it is judged that all the water has been removed, put the 
dish in a desiccator (Fig. 56), let it cool, and then weigh. Zinc chloride 
is deliquescent. Hence the dish and contents must be weighed 
quickly. It is hardly possible to get weights which agree, but the 
variation should not be much. 

The equivalent of chlorine is 35.5. Calculate the equivalent of 
zinc to chlorine. Submit the result to the Teacher before removing 
the contents from the dish. 

Required Exercises. — As in Exp. 88. 

IONS AND IONIZATION 

(Practical Chemistry, pp. 201-216, §§ 230-247) 

Experiment 94 — Electrolytes and Non-Electrolytes 

(Demonstration Experiment) 

Object. — To find out whether a substance forms a conducting or a non¬ 
conducting solution. 

Materials. — Hydrochloric acid, sodium hydroxide, calcium chloride, 
sugar, alcohol, glycerin. 



Fig. 56. — A desiccator 
for keeping zinc chlo¬ 
ride dry 








§8 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Apparatus. — As in Fig. 57. A is a beaker for the solution, B and C are 
electrodes (of aluminium or platinum) which are supported on the top 
of the beaker by a strip of wood. D is an electric light bulb which is 
connected with the wire from the electrode B and with one end of the 
wire E. The wire from the electrode C and the other end of the wire 
E are connected with the street current (reduced) or with a storage 
battery. 


a. Construct and ar¬ 
range the apparatus as 
in Fig. 57. Fill the 
beaker two-thirds full of 
dilute hydrochloric acid, 
see that all connections 
are tight, and turn on 
the current. Does the 
bulb glow ? Why ? 



b. Proceed as in a, 
using successively solu¬ 
tions of sodium hydrox¬ 
ide, calcium chloride, 


Fig. 57. — Apparatus for showing what solu¬ 
tions conduct electricity 


sugar, alcohol, and glycerin. Clean the beaker each time. Observe 
and state each result. 

Answer: 1. What substances form solutions which conduct electricity? 

2. What substances form non-conducting solutions? 

3. What is the name of the classes of substances in 1 ? In 2 ? 

Experiment 95 — Chemical Behavior of Solutions of Salts 

Materials. — For a, solutions of silver nitrate, silver sulphate, and chlorides 
of ammonium, barium, calcium, magnesium, sodium, and potassium; 
potassium chlorate, potassium perchlorate. For c, solutions of barium 
chloride, barium nitrate, sulphates of copper, sodium, aluminium, mag¬ 
nesium, and zinc. 

a. Test separately a dilute solution of the substances enumerated 
under a by adding a few drops of silver nitrate solution. State the 
result in each case. 

b. Add a few drops of silver sulphate solution to several of the 
solutions used in a. State the result. 

c. Test separately a dilute solution of substances enumerated 
under c, by adding to each a few drops of barium chloride solution. 
State the result in each case. 
















IONS AND IONIZATION 


d. Proceed as in c, using a few drops of barium nitrate solution 
in place of barium chloride. 

Required Exercises. — i. What ion is common to solutions of chlo¬ 
rides? Of sulphates? 

2. Explain the general result in a in terms of the theory of ionization. 
Also the results in b. 

3. What ion is in solutions of all barium salts? All silver salts? 

4. What ion other than hydrogen is in a solution of sulphuric acid? 
What ion other than potassium ion is in a solution of potassium chlorate ? 
Of potassium perchlorate ? 

5. What ion is in solutions of all acids? Of all bases? Of all sodium 
salts ? 

6. Make a list df the salts used in the whole experiment and their cor¬ 
responding ions, indicating the ions by name and formula. 


Experiment 96 — Electrolysis of Copper Sulphate Solution 
— Short Method 

(Demonstration Experiment) 

Material. — Dilute copper sulphate solution. 

Apparatus. — Small battery jar (or beaker), two electrodes (pieces of 
electric light carbon) and connection wires, battery of four or more 
cells (or other source of electric current). 

Fill the battery jar about two-thirds full of dilute copper sulphate 
solution. Wind the end of a piece of the wire around one end of each 
electrode and hang the electrodes in the solution by bending the wire 
over the edge of the jar (or supporting them by a strip of wood which 
rests across the top of the jar). Connect the ends of the wires with 
the battery. 

Before turning on the current (or making the final connection ) t 
examine each electrode and note the absence of a deposit. Turn on 
the current and observe at which electrode bubbles of gas form. Let 
the current run about ten minutes, and then examine each electrode. 
Compare with their appearance before the electrolysis took place. 
Upon which electrode (anode or cathode) is there a deposit? What 
is the deposit? 

Sketch the apparatus, and describe the electrolysis of copper sul¬ 
phate in terms of the theory of ionization, using the sketch in your 
interpretation. 


go 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 97 — Electrolysis of Copper Sulphate Solution 
— Long Method 


(Demonstration Experiment) 


Materials. — Copper sulphate solution, joss stick. 


Fill the Hofmann 




apparatus (Fig. 58) full of copper sulphate solu¬ 
tion. Connect with a reduced street current 
or a storage battery. Turn on the current 
and let it run until about 10 cc. of gas collects. 

At which electrode (anode or cathode) was 
a gas liberated? A solid deposited? Have a 
glowing joss stick ready, let out a little gas, and 
test it with the glowing joss stick. What is 
the gas ? What is the solid ? 

Answer: 1. What ions are in copper sulphate 
solution ? 

2. To what electrode does each kind of ion mi¬ 
grate? 

3. What happens when the ions reach the elec¬ 
trodes? 

4. What secondary action takes place at one elec¬ 
trode ? 

Experiment 98 — Electrolysis of Sodium 
Sulphate Solution 

(Demonstration Experiment) 


Fig. 58. —Hofmann Materials. — Sodium sulphate solution, neutral 
apparatus for litmus solution, joss stick, wax taper, 
showing electrol) - jqq t p e Hofmann apparatus (Fig. 58) full of 
sodium sulphate solution colored with neutral 
litmus solution. Proceed as in Exp. 97. Let the current run until 
the smaller volume of gas measures about 10 cc. Observe the color 
of the solution in each tube; also the relative quantity of gas. Test 
the gases as in Exp. 49. State the result. Interpret the electroly¬ 
sis of sodium sulphate by the theory of ionization. 


Answer: 1. What is the name of each gas? 

2. At which electrode was each gas liberated? 

3. Why was the color changed in each tube? 

















IONS AND IONIZATION 


9i 


Experiment 99 — Electrolysis of Potassium Iodide Solution 

(Demonstration Experiment) 

Materials. — Starch, potassium iodide. 

Apparatus. — Sheet of metal (tin or irori), battery of two or more cells. 

Grind together in a mortar a lump of starch and a crystal of potas¬ 
sium iodide. Add enough water to make a thin liquid. Dip a piece 
of filter paper into the mixture, and spread the wet paper upon the 
sheet of metal. Press the end of one wire upon the metal, and 
draw the end of the other wire across the sheet of paper. Observe 
the result. If there is no result, reverse the ends of the wires. The 
dark marks are caused by iodine which is liberated from the potas¬ 
sium iodide and colors the starch. 

Required Exercises. — i. Describe briefly this experiment. 

2. Iodine is a non-metal. Are iodine ions anions or cations? At what 
electrode is iodine liberated? 

Experiment 100 — Dissolved Substance and Boiling Point 

Materials. — Sodium chloride, sugar (both finely powdered). 

Apparatus. — Thermometer, 250 cc. Erlenmeyer flask. 

a. Stand a 250 cc. Erlenmeyer flask on a gauze-covered ring at¬ 
tached to an iron stand and clamp it about the neck. Pour 100 cc. 
of water into the flask, heat the water to boiling, hold the thermom¬ 
eter in the steam a minute or two, then lower it into the water, and 
observe the highest temperature. Record, and call this the boiling 
point. 

Remove the burner, and carefully slide 10 gm. of sodium chloride 
from a creased paper into the flask, taking care not to let any of the 
solid stick to the inside of the flask. Heat to boiling, and as soon as 
the solution boils steadily, observe and record the temperature. In 
the same way add another 10 gm. portion of sodium chloride, and 
find the boiling point of the solution. 

Compare the three boiling points. What effect has dissolved 
sodium chloride on the boiling point of water? 

b. Proceed as in a, using finely powdered sugar in place of sodium 
chloride. Compare the general result with a. 

Answer: 1. What effect has a dissolved substance on the boiling point 
of water? 

2. Does the effect differ with the substance (in comparable solutions)? 
How? Why? 


92 EXPERIMENTS IN PRACTICAL CHEMISTRY 


3. Does the effect differ with the quantity of the substance (in the same 
quantity of water) ? How? Why? 

4. Suppose a mole of sugar were dissolved in 1000 gm. of water, how 
would it affect the boiling point? Would the effect of a mole of sodium 
chloride be the same or different? Why? 

Experiment 101 — Dissolved Substance and Freezing Point 

Materials. — Ice, finely powdered sodium chloride and sugar. 

Apparatus. — Bottle, thermometer. 

a. Fill the bottle one-third full of cold water, drop in several small 
pieces of ice, and shake well. Insert the thermometer, stir, and ob¬ 
serve the lowest temperature. Make at least three readings. Re¬ 
cord the temperatures. Call the lowest one the freezing point of 
water (although it may be a little higher than the actual freezing 
point). 

Carefully slide 10 gm. of sodium chloride into the bottle, shake 
a minute or two, then stir with the thermometer, and observe and re¬ 
cord the lowest temperature. Proceed in the same way with another 
10 gm. portion of sodium chloride. 

Compare the lowest temperatures. Compare them with the lowest 
temperature of the water. What effect has dissolved sodium chloride 
on the freezing point of water? 

b. Proceed as in a, using sugar in place of sodium chloride. Com¬ 
pare the general result with a. 

Answer: 1. Apply 1 in Exp. 100 to the freezing point of water. 

2, 3, 4. As in Exp. 100. 

Experiment 102 — Colored and Colorless Ions 

Materials. — Solutions (dilute) of copper sulphate, copper nitrate, cop¬ 
per bromide, nickel chloride, nickel sulphate, cobalt chloride, cobalt 
nitrate, potassium dichromate, ammonium dichromate, sodium dichro¬ 
mate, potassium chromate, potassium permanganate — prepared for 
the class. 

a. Observe and state the color of the copper solutions. To what 
ion is the color due? Give its ionic name and formula. Are the 
other ions in the copper solutions colored or colorless? What is a 
simple proof of your answer? 

b. As in a with the nickel, etc., solutions. 

Required Exercises. — 1. Write the formula of each substance and 
the corresponding ions. 


SULPHUR — SULPHIDES 


93 


2. Make a list of colored ions. 

3. Make a list of 10 colorless anions. Of 10 colorless cations. 

Experiment 103 — Ionization and Concentration 

(Demonstration Experiment) 

Apparatus. — Oblong battery jar or deep dish, carbon electrodes which 
reach to the bottom of the jar, separatory funnel (100 cc.), source of 
electric current ( e.g . street current — direct), and two 40-watt bulbs. 

a. Fill the jar nearly full of water. Insert the electrodes in the 
water, put the two bulbs in the circuit, make the proper connections, 
and turn on the current. Note the effect on the bulbs. Turn off 
the current. 

b. Put about 50 cc. of concentrated sulphuric acid in the separa¬ 
tory funnel, let enough run out to fill the stem, and quickly lower the 
stem into the water until the end rests on the bottom of the jar. Let 
the acid run in slowly beneath the water. Lift out the funnel. Turn 
on the current. Note the effect on the bulbs. Compare with a. 

c. Stir the acid slowly into the water and note the result, as in b. 
Compare with a and b. 

Required Exercises. — 1. Describe the experiment (using a sketch of 
the apparatus). 

2. What does this experiment show about the comparative conductivity 
of water, concentrated sulphuric acid, and dilute sulphuric acid? 

3. In which is there greater ionization, concentrated or dilute sulphuric 
acid? 

4. How does this experiment show the relation of ionization to 
concentration ? 


SULPHUR — SULPHIDES 

(Practical Chemistry, pp. 218-227, §§ 248-258) 

Experiment 104 — Physical Properties of Sulphur 

Materials. — Brimstone, flowers of sulphur, lump of sulphur, thread. 
Apparatus. — Graduated cylinder (500 cc.). 

a. Examine and describe specimens of brimstone and flowers of 
sulphur. 

b. Tie a thread around a lump of sulphur, and weigh it on the 
scales. Slip it carefully into a graduated cylinder (Fig. 59) previ¬ 
ously filled with water to a known point. Note the increase in the 
volume of water. The increase in volume equals the volume of the 


94 EXPERIMENTS IN PRACTICAL CHEMISTRY 


cc 


sulphur. Calculate the specific gravity by: Sp. gr. = Wt. of sul¬ 
phur -7- Wt. of equal vol. of water. State the result. 

c. Fill a test tube one-fourth full of small 
lumps of sulphur, attach the test tube holder, 
and heat until all the sulphur is melted. Ob¬ 
serve the color and consistency. Heat intensely, 
and observe the result. Continue to heat until 
the sulphur boils and then observe as before. 
Let the test tube cool, and save it for Exp. 108. 
Summarize the effects of heating sulphur. 

Note. — If the test tube should break during the 
heating, extinguish the burning sulphur with sand. 


Experiment 105 


- Chemical Properties of 
Sulphur 


Fig. 59. — Appa- Materials. — Sulphur, iron thread. 

ratus for finding Set £ re to a sulphur i n a deflagrat- 

the specific grav- . , . . ^ 

ity of sulphur in g spoon, and lower the spoon into a bottle. 

Cautiously waft the fumes toward the nose, and 
observe and describe the odor. What is the product of burning 
sulphur ? 

b. Fill a test tube one-fourth full of iron thread, and add an equal 
bulk of flowers of sulphur. Heat the part containing the sulphur —• 
gently at first and then intensely until there is marked evidence of 
chemical action. Remove the test tube from the flame as soon as the 
action begins. Observe and describe the result. What is the name 
of the product of the chemical change? 


Experiment 106 — Orthorhombic (Rhombic) Sulphur 

Materials. — Powdered roll sulphur, carbon disulphide. 

Apparatus. — Lens. 

Put about 2 gm. of powdered roll sulphur in a test tube and add 
about 5 cc. of carbon disulphide — remember to keep the carbon 
disulphide away from flames. Shake until most of the sulphur is 
dissolved, then filter the solution (or pour the clear liquid) into an 
evaporating dish to crystallize. Stand the dish in the hood or out 
of doors, where there is no flame and where the offensive vapor will 
be quickly removed. Allow the liquid to evaporate; watch the 
crystallization toward the end, if convenient, and remove and dry 
the best crystals. 







SULPHUR — SULPHIDES 


95 


Examine the crystals with the eye and with a lens. Note the 
color, luster, and shape. Draw the best shaped one. 

Experiment 107 — Preparation of Monoclinic Sulphur 

Materials. — Sulphur (roll), carbon disulphide. 

a. Fix a folded filter paper firmly in a funnel, and place the fun¬ 
nel in a test tube which stands in a rack. Fill a test tube two-thirds 
full of roll sulphur, heat it at first throughout its length, and gradu¬ 
ally increase the heat until all the sul¬ 
phur is melted. Then quickly pour it 
upon the filter paper. Let it cool until 
crystals appear just below the surface, and 
then pour out the remaining melted sul¬ 
phur at once into a dish of water. 

Remove the paper and adhering sul¬ 
phur, and cut, or break, open the cone 
of crystallized sulphur (Fig. 60). Observe 
and record the properties of the crystals, especially the shape, size, 
color, luster, and brittleness. Allow the best crystals to remain un¬ 
disturbed for a day or two; then examine again, and record any 
marked changes. 

Experiment 108 — Amorphous (Plastic) Sulphur 

Materials. — Sulphur, or test tube and contents from Exp. 104 c. 

Put a few pieces of roll sulphur in a test tube, or use the test tube 
saved in Exp. 104 c, heat carefully until the sulphur boils, and then 
quickly pour the molten sulphur into a dish of cold water. This is 
the plastic variety of amorphous sulphur. Note its properties. 
Compare with orthorhombic and monoclinic sulphur. 

Preserve, and examine it after twenty-four hours. Describe it, 
and compare its properties with those previously observed. Pul¬ 
verize a small piece and test its solubility in carbon disulphide. State 
the result. 

Experiment 109 — Hydrogen Sulphide — Short Method 

Materials. — Ferrous sulphide, dilute hydrochloric acid, lead nitrate 
solution. 

Apparatus. — As in Fig. 61 for d. 

Caution. — Perform this experiment in the hood. 



Fig. 60. — Monoclinic 
sulphur 


g 6 experiments in practical chemistry 


Slip a small piece of ferrous sulphide carefully into a test tube, 
add 5 cc. of dilute hydrochloric acid, and cau¬ 
tiously note the odor of the gas. Describe the 
odor. 

b. Wet a piece of filter paper with lead nitrate 
solution and hold it in the escaping gas. Note 
the change in color. Into what lead compound 
has the lead nitrate been changed ? 

c. Add a little more ferrous sulphide and di¬ 
lute hydrochloric acid to the test tube, and hold 
a lighted match at the mouth of the tube. 
Observe the result. Cautiously note the odor 
of the gas. What is the gas ? 

d. Arrange an apparatus as in Fig. 61. Fill 
B half full of water. Put ferrous sulphide and 
dilute hydrochloric acid in the test tube A 



Fig. 6i. — Appara¬ 
tus for preparing 
hydrogen sul¬ 
phide water 


and let the gas bubble through the water in the test tube B for a few 
minutes. Use the solution in Exp. in. Cork it tightly unless it 
is to be used soon. 


Experiment 110 — Hydrogen Sulphide — Long Method 

Materials. — Ferrous sulphide, dilute hydrochloric acid. 

Apparatus. — As in Fig. 62 ; stoppered bottle. 


Caution. — Hydrogen sul¬ 
phide is a poisonous gas and 
has an offensive odor. It 
should not be inhaled nor al¬ 
lowed to escape into the labora¬ 
tory. All experiments with 
hydrogen sulphide should be 
performed in the hood. 

I. Preparation. — Construct 
and arrange an apparatus like 
that shown in Fig. 62. Put 10 
gm. of coarsely powdered fer¬ 
rous sulphide in the bottle A, 
insert the stopper tightly, and 
adjust the apparatus so that 
the end of the delivery tube 
pneumatic trough. Introduce a 
the dropping tube. Hydrogen 



Fig. 62. — Apparatus for preparing 
hydrogen sulphide 

will be under the support of the 
little dilute hydrochloric acid through 
sulphide is rapidly evolved. If the 































SULPHUR — SULPHIDES 


97 


evolution of gas slackens or stops, add more hydrochloric acid. Col¬ 
lect three bottles, removing each as soon as full and covering tightly 
with a piece of dry filter paper. Set aside until needed. When all 
the bottles have been filled with gas, proceed at once with II. 

II. Properties. — a. Waft a very little of the gas cautiously to¬ 
ward the nose, and describe the odor. This odor is characteristic 
of hydrogen sulphide, and is a decisive test. Has the gas color? 

b. Test the gas from the same bottle with both kinds of moist 
litmus paper. Is hydrogen sulphide acid, alkaline, or neutral? 

c. Hold a lighted match at the mouth of the same bottle. Ob¬ 
serve the color of the flame. Observe cautiously the odor of the prod¬ 
uct of the burned gas; to what compound is the odor due? What, 
then, is one constituent of hydrogen sulphide? 

d. Burn another bottle of hydrogen sulphide and hold a cold, dry 
bottle over the burning gas. What additional experimental evidence 
does this result give regarding the composition of hydrogen sulphide ? 

e. Pour several drops of concentrated nitric acid into a bottle of 
hydrogen sulphide, cover, and shake. Note the solid product. What 
is it ? Explain its formation. 

Required Exercises. — i. Summarize briefly the properties of hy¬ 
drogen sulphide gas. 

2. State the experimental evidence of its composition. 

Experiment 111—Preparation and Properties of Sulphides 

Materials. — Hydrogen sulphide water, clean copper wire, clean sheet 
lead, bright silver coin, lead oxide (litharge); solutions of lead nitrate, 
arsenic trioxide (in hydrochloric acid), tartar emetic, zinc sulphate, 
cadmium nitrate, silver nitrate, and mercuric chloride {Poison!). 

a. Obtain a bottle half full of hydrogen sulphide water, and hang 
(by a wire or thread) inside the bottle (i) a clean copper wire, (2) a 
clean strip of lead, and (3) a bright silver coin. Describe the result 
in each case. The products are sulphides of the respective metals; 
give the name and formula of each. 

b. Put a little litharge — the brownish yellow oxide of lead — in 
a test tube, cover it with hydrogen sulphide water, and warm gently. 
The product is lead sulphide. Describe it. 

c. Add hydrogen sulphide water to lead nitrate solution. De¬ 
scribe the product. What is the name of the product ? 

d. Proceed as in c with the arsenic solution. Observe the color 
of the product. Compare with c. What is the product? 

e. Proceed as in c with the tartar emetic solution. Tartar emetic 


g8 EXPERIMENTS IN PRACTICAL CHEMISTRY 


is a compound of antimony. Observe the color of the product. Com¬ 
pare with c and d. What is the product? 

f. Proceed as in c with the zinc sulphate solution. Observe the 
color of the product. Compare with c, d, and e. What is the prod¬ 
uct? 

g. Proceed as in c with solutions of cadmium nitrate, silver nitrate, 
and mercuric chloride (Poison!). Use separate test tubes. Observe 
the color in each case, and name the product. 

Required Exercises. — i. Prepare a list of sulphides, including the 
name, formula, and color of each. 

2. Write the equation for the interaction of (a) lead nitrate and hydro¬ 
gen sulphide, ( b ) arsenic trichloride and hydrogen sulphide. 

3. Write the equations in 2 in ionic form. 

4. How could hydrogen sulphide be used to identify the metallic part • 
of many salts? 

5. Suggest a test for sulphide ions. 

SULPHUR DIOXIDE — SULPHUROUS AND 
SULPHURIC ACIDS — SULPHITES AND SULPHATES 

(Practical Chemistry, pp. 229-241, §§ 259-276) 

Experiment 112 — Sulphur Dioxide — Short Method 

Materials. — Sulphur, joss stick, litmus paper, potassium permanganate 
solution (dilute), colored flower. 

Apparatus. — Bottle fitted with cork. 

Caution. — Perform this experiment in the hood. 

Fill a deflagrating spoon with sulphur, set it afire, and lower the 
spoon into a bottle. In a minute or two, remove the spoon, and 
cover the bottle with a glass plate or (tightly) with a piece of filter 
paper. In the same way prepare and cover two more bottles of sul¬ 
phur dioxide. 

a. Cautiously note the odor. After the smoke (which is not sul¬ 
phur dioxide) has settled, observe whether the gas has any color. 

Is it heavier or lighter than air? Save for b. 

b. Hold a blazing joss stick or a burning match in the bottle of 
gas saved from a. Does the gas burn? Does it support combus¬ 
tion? 

c. Stand the second bottle of gas mouth downward in a vessel 
of water (e.g. pneumatic trough). Shake, still keeping the mouth 
submerged. Observe the result. What does the result show about 


SULPHUR DIOXIDE 


99 


the solubility of sulphur dioxide in water ? Slip a piece of filter paper 
under the mouth of the bottle, remove, invert, and test the liquid 
with litmus paper. State the result. To what compound is the re¬ 
sult due? Save for d. 

d. Pour a few drops of very dilute potassium permanganate solu¬ 
tion into the bottle saved from c, and shake well. Compare the 
color of the two liquids. If the result is not satisfactory, repeat, 
and use a bottle full of sulphur dioxide to which only 5 cc. of water 
has been added. Explain the chemical change. 

e. Moisten a few petals of a colored flower with water, put them 
in the third bottle of sulphur dioxide, and insert the cork. Observe 
and describe any change in color. 


Experiment 113 — Sulphur Dioxide and Sulphurous Acid 


gm. of 


Materials. — Sodium sulphite, dilute sulphuric acid, litmus paper, joss 
stick, colored flower, potassium permanganate solution. 

Apparatus. — As in Fig. 63. 

Caution. —■ Perform this experiment in the hood. 

I. Preparation. — a. Sulphur Dioxide. — Put about 10 
sodium sulphite in the flask, and insert 
the stopper with its tubes. Adjust the 
apparatus as shown in Fig. 63. Fill the 
cup with dilute sulphuric acid, press the 
pinch-clamp a little, and let the acid 
flow drop by drop upon the sodium sul¬ 
phite. Sulphur dioxide is evolved and 
passes into the bottle, which should be 
removed when full, as previously de¬ 
scribed. Warm gently, if the action 
slackens. Moist blue litmus paper held 
for an instant at the mouth of the bot¬ 
tle will show (by change in color) when 
the latter is full. Collect two bottles of 
gas, cover each tightly with a piece of 
filter paper or a glass plate, and set aside 
until needed for II a. 

b. Sulphurous Acid. — As soon as 
the second bottle of gas has been re¬ 
moved and covered, put in its place a 
bottle one-fourth full of water. Adjust its height (if necessary) by 
wooden blocks, so that the end of the delivery tube is just above the 



Fig. 63. — Apparatus for 
preparing sulphur dioxide 
and sulphurous acid 




















100 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


surface of the water. Continue to add the acid and to heat at inter¬ 
vals. Shake the bottle occasionally. When II a, etc., have been 
done, proceed with this solution as in III a, etc. 

II. Properties of Sulphur Dioxide Gas. a, b, c, d, e. Proceed 
as in Exp. 112 a, b, c, d, e. 

III. Properties of Sulphurous Acid. — a. Observe the odor and 
the taste cautiously. State each result. 

b. Apply the litmus test, and state the result. 

c. Drop a short piece of magnesium ribbon into 10 cc. of the solu¬ 
tion. Warm slightly if there is no action. State the result. 

d. Add a few drops of potassium permanganate solution to 5 cc. 
of sulphurous acid. Observe and state the result. What chemical 
change has the sulphurous acid undergone ? 

e. Put about 10 cc. of sulphurous acid in an evaporating dish, 
support the dish on a gauze-covered ring attached to an iron stand, 
heat in the hood, gradually, and note the odor of the liberated gas. 
Blow the gas out of the dish frequently, and then smell of the liquid. 
Boil until most of the liquid is evaporated, and test the remainder 
with litmus paper. What effect has heat on sulphurous acid? 

f. Put 10 cc. of sulphurous acid into a test tube, cover loosely, and 
let it stand exposed to the air for a day or two. Add 10 cc. of water, 
boil for a minute or two, and test as in Exp. 115 b. State and ex¬ 
plain the result. 

g. Put 10 cc. of sulphurous acid in a test tube, add 2 cc. of con¬ 
centrated nitric acid, and boil gently for a minute or two. Add 
about 10 cc. of water, shake, and test as in Exp. 115 b. State and 
explain the result. Compare with d and f. 

Experiment 114 — Properties of Sulphuric Acid 

Materials. — Concentrated sulphuric acid, thin stick of wood, sugar. 
Apparatus. — Graduated cylinder (100 cc.), hydrometer for heavy liquids. 

Caution. — Concentrated sulphuric acid is a corrosive liquid. Do 
not spill it on the flesh or clothing. 

a. Weigh a 25 cc. graduated cylinder, pour in concentrated sul¬ 
phuric acid to a convenient height (e.g. 20 cc.) and weigh again. Read 
the exact volume of the acid. From the weight and volume of the 
acid, calculate its specific gravity. 

Find the specific gravity of a sample of the same acid by reading 
the hydrometer which floats in the acid (Fig. 64). (This apparatus 
should be arranged for the class by the Teacher. See Exp. 38.) 

b. Add an equal volume of concentrated sulphuric acid to a test 


SULPHURIC ACID 


IOI 


tube one-fourth full of water, shake well, and observe at once the 
change in temperature by holding the tube in the hand. Save the 
solution for c and d. 


c. Dip a glass rod into the sulphuric acid from b and write some 
letters or figures on a sheet of paper. Move 

the paper back and forth slowly over a low 
flame, taking care not to set fire to the paper. 

As the water evaporates the dilute acid be¬ 
comes concentrated. Observe and describe 
the result. (Paper is largely a compound of 
carbon, hydrogen, and oxygen, and the hydro¬ 
gen and oxygen are present in the proportion 
to form water.) Explain the general chem¬ 
ical change in this experiment. 

d. Warm the acid in the test tube saved 
from b, stand a stick of wood in the acid, and 
allow it to remain for fifteen minutes or more. 

Then remove the stick and wash off the acid. 

Describe and explain the change in the wood. 

e. Put 5 gm. of sugar in an evaporating 
dish, add just enough warm water to make a 
thick sirup, and stand the dish on a block of 
wood (or in the sink). Cautiously pour 5 or 
10 cc. of concentrated sulphuric acid upon the 
liquid. Stand back and observe the result. 




Fig. 64. — Finding 
the specific gravity 
of sulphuric acid 
with the hydrometer 


Explain the result. 


Experiment 115 — Tests for Sulphuric Acid, Sulphates 
(Soluble and Insoluble), and S0 4 -ions 

Materials. — Sulphuric acid, sodium sulphate, barium chloride solution, 
calcium sulphate, charcoal, powdered charcoal, silver coin. 
Apparatus. — Blowpipe and blowpipe tube. 

a. Sulphuric Acid. — Recall a test for concentrated sulphuric 
acid. How could the same test be utilized for dilute sulphuric acid ? 

b. Sulphuric Acid and Soluble Sulphates, i.e. solutions containing 
S 0 4 -ions. — Add barium chloride solution to the solution of the acid 
or the sulphate, and boil with dilute hydrochloric acid. If no sul¬ 
phur dioxide gas is liberated and an insoluble precipitate remains, 
the original solution contained SCVions. 

c. Insoluble Sulphates. — Proceed as in Exp. 134 A b, using cal¬ 
cium sulphate (or any sulphate insoluble in water). 






102 EXPERIMENTS IN PRACTICAL CHEMISTRY 


CARBON — CARBONIC ACID — CARBONATES 
— OXIDES 

(Practical Chemistry, pp. 244-258, §§ 277-295) 


Experiment 1!6 — Properties of Graphite 


Materials. — Graphite, thread, articles for d. 
Apparatus. — Graduated cylinder (500 cc.), test wire. 



a. Rub a piece, of graphite with the finger, 
and describe the feeling. Draw a piece slowly 
across a sheet of paper, and state the result. 

b. Proceed with a lump of graphite as in 
Exp. 104 b (Fig. 65). Record the result. 

c. Wind the end of a test wire around a small 
piece of graphite and hold it in the hottest part 
of the flame for five or ten minutes (Fig. 66). 
State the result. 

d. Examine stove polish, plumbago crucible, 
core of a lead pencil, electrodes, or lubricant. 
How would you test them for graphite? 


Fig. 65. — Appa¬ 
ratus for finding 
the specific grav¬ 
ity of graphite 


Experiment 117 — Properties of Charcoal 


Apparatus. 


Materials. — Wood charcoal (lump and powder), 
animal charcoal, copper wire, crucible, vinegar, hy¬ 
drogen sulphide solution. 

Test tube fitted with a cork, crucible and support. 


Wood charcoal. — Wind the end of 
a test wire around a piece of charcoal, 
hold it in the flame, and observe the 
result, especially the ease or difficulty 
of ignition, presence or absence of 
flame and smoke, formation of ash. 
Compare with graphite (Exp. 116 c). 

Animal charcoal. — a. Cover the 
bottom of a crucible with animal char¬ 
coal, stand the crucible on a triangle 



Iig. 66 . — Apparatus for heat¬ 
ing graphite in a hot flame 


and heat intensely for about half an hour. Examine the residue. 
What is it? 

b. Fill a test tube one-fourth full of powdered animal charcoal 
(refer to Fig. 5). Add 10 cc. of hydrogen sulphide solution, and 












CARBON — CARBONATES 


103 


cork securely. Shake well. After ten minutes, remove the stopper 
and smell of the contents. Is the odor much less offensive? What 
property of animal charcoal does this experiment illustrate? 

c. Fill a test tube one-fourth full of powdered animal charcoal, 
(refer to Fig. 5), add 10 cc. of vinegar, shake thoroughly for a 
minute, and then warm gently. Filter through a wet paper. Com¬ 
pare the colors of the filtrate and the original vinegar. Describe 
briefly. What property of animal charcoal does this experiment 
illustrate ? 


Experiment 118 — Testing for Carbon 

Test various substances for carbon by heating in a test tube or a 
crucible, as in Experiment n e. State the result. 

Experiment 119 — Reduction of Copper Oxide by Carbon 

Materials. — Powdered copper oxide, powdered wood charcoal, calcium 
hydroxide. 

Apparatus. —■ As in Fig. 67, lens. 

Grind together in a mortar about 5 
gm. of copper oxide and 1 gm. of wood 
charcoal. Put the mixture on a creased 
paper (refer to Fig. 5) and slip it into 
the test tube A. Fill the bottle B half 
full of calcium hydroxide. Arrange the 
apparatus as in Fig. 67. 

Heat the test tube gently at first, 
and adjust the height so the evolved 
gas will bubble through the calcium 
hydroxide in B. Heat intensely for 
about ten minutes, moving the burner 
along the part of the test tube that con¬ 
tains the mixture. Observe the change 
in the calcium hydroxide. To what is 
the change due? 

As soon as a definite change is noted in B, remove the end of the 
delivery tube from B, and stop heating. Let the test tube cool and 
pour the contents into a mortar. Examine it carefully with the eye 
and with a lens. What is detected besides carbon? 

Interpret the chemical change and write the equation for the re¬ 
action. 



Fig. 67. — Apparatus for re¬ 
ducing copper oxide with 
carbon 










104 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 120 — Carbonic Acid 

(Demonstration Experiment) 

Materials. — Solutions of sodium hydroxide and phenol-phthalein. 
Apparatus- — Carbon dioxide generator with washing tube. 

Construct and arrange the carbon 
dioxide generator like that shown in 
Fig. 68. (A bottle may be used in 
place of the test tube A.) Put 
marble chips in A and water in B 
(to wash the gas free from acid). 
Use dilute hydrochloric acid. Fill a 
bottle half full of water, add a few 
drops of phenol-phthalein solution 
and just enough sodium hydroxide 
solution to color the liquid a faint 
pink (after shaking). Pass a slow 
current of carbon dioxide from the 
generator through the liquid in the 
is produced in the absorbing liquid. 

Experiment 121 — Normal and Acid Calcium Carbonate 

(Demonstration Experiment) 

Apparatus. — Carbon dioxide generator (as in Exp. 120). 

Fill the bottle C one-fourth full of calcium hydroxide solution and 
pass carbon dioxide through it until the precipitate at first formed 
disappears. Filter, if the liquid is not perfectly clear. Put 15 cc. 
into a test tube and heat gently. Observe all the changes. State 
the results of heating the clear solution. 

Required Exercises. — 1. What is the name of the first precipitate? 

2. Into what soluble compound was this precipitate formed by inter¬ 
action with carbon dioxide? 

3. Into what was the soluble compound formed by heating? 

4. Write equations for (1) preparation of carbon dioxide, (2) forma¬ 
tion of the precipitate, (3) formation of the soluble compound, (4) decom¬ 
position of the soluble compound. 

Experiment 122 — Testing for Carbonates 

Materials. — Barium hydroxide solution, baking soda, washing soda, 
baking powder, native chalk, tooth powder, white lead, whiting, old 
mortar (or plaster), “unknowns.” 



Fig. 68 . — Apparatus for pre¬ 
paring and washing carbon 
dioxide 


bottle until a definite change 
Describe and explain it. 






















CARBON — CARBONATES 


105 

Put some of the fine solid in a test tube, add a little water and dilute 
hydrochloric acid, and shake. Then hold a glass tube, which has 
been dipped into barium hydroxide solution, inside the test tube for 
a minute or two about 3 cm. above the mixture. If the action is 
not marked, gently warm the test tube. State the result in each 
case. 


Experiment 123 — Carbon Monoxide 


(Demonstration Experiment) 

Materials. — Oxalic acid, calcium hydroxide solution. 

Apparatus. — As in Fig. 69. - 

Caution. — Carbon monoxide and oxalic acid are poisonous. Hot 
sulphuric acid is dangerous. Perform this experiment in the hood 
with unusual care. 

I. Preparation. — Put 10 gm. of 
oxalic acid in the flask A (Fig. 69), 
and add 25 cc. of concentrated sul¬ 
phuric acid. Put enough calcium 
hydroxide solution in B to cover the 
end of the tube E. Arrange the ap¬ 
paratus as in Fig. 69. The end of H 
should rest on the bottom of the 
pneumatic trough just beneath the 
hole in the sup¬ 
port. 

Heat the flask 
A gently, and car¬ 
bon monoxide will 
be evolved. Col¬ 
lect all the gas, but 
do not use the first 
bottle, covering the Fig - 6 9 - ~~ Apparatus for preparing carbon monoxide 

bottles with glass plates as they are filled, and setting them aside 
temporarily. When the last bottle has been collected and covered, 
loosen the stopper in B, and remove the end of H from the water in 
the trough. Proceed at once with II. 

II. Properties. — a. Note that the gas is colorless. 

b. Hold a lighted match at the mouth of a bottle. Note the flame, 
especially its color. After the flame has disappeared, drop a lighted 
match into the bottle. Describe the result. Draw a conclusion 
and verify it by c. 

























io6 EXPERIMENTS IN PRACTICAL CHEMISTRY 


c. Burn another bottle of gas, note the flame again, and after the 
flame has disappeared pour calcium hydroxide solution into the bot¬ 
tle and shake. Explain the result. 

Required Exercises. — i. Describe briefly the preparation of car¬ 
bon monoxide. 

2. Summarize the observed properties of carbon monoxide. 

3. What gas besides carbon monoxide was produced in I? 


FUELS — ILLUMINATING GAS — FLAME 

(Practical Chemistry, pp. 260-288, §§ 296-338) 


Experiment 124 — Composition of Fuels 


Materials. — Soft coal, wood, alcohol, gasolene, calcium hydroxide solu¬ 
tion. 

Apparatus. —- Crucible (porcelain or iron). 


a. Put a little powdered soft coal in a test tube, attach the holder, 
and heat intensely in the flame (Fig. 70). Note the formation of 

moisture and volatile matter (smoke). 
Describe the result. 

b. Optional. Put a little powdered 
soft coal in a crucible (porcelain or 
iron), support the crucible on a tri¬ 
angle (Fig. 71), and heat intensely. 
After the smoking has stopped, note 
the black, hard mass of fixed carbon. 
Continue to heat until the carbon has 
disappeared. The residue is ash (or 
ashes). Describe it. 

c. Proceed as in a, using shavings 
or small pieces of wood. Describe 

the result. Continue to heat until the carbon is burned. Is ash 
left? 



Fig. 70. — Heating soft coal to 
detect volatile matter 


d. Put several drops of alcohol in a dish, set it afire, and hold a 
cold, dry bottle over the flame. When the flame goes out, remove 
the bottle, and stand it mouth upward on the desk. What is the 
film inside the bottle? Add calcium hydroxide solution, cover the 
bottle with the hand, shake well, and note the result. What do these 
two tests show about the composition of alcohol? 

e. Proceed as in d, using gasolene instead of alcohol (Care 0 

f. Hold a cold dry bottle for a minute or two over a small Bunsen 
flame. Note the obvious product. What is it ? What is the other 







FUELS — ILLUMINATING GAS — FLAME 


107 

product? Verify your answer by a simple test. Apply thq last 
question asked in d. 

Experiment 125 — Analysis of Coal 

Object. — To find the per cent of moisture, volatile matter, fixed carbon, 
and ash in a sample of coal. 

Material. — Coal (powdered very fine). 

Apparatus. — 2 crucibles, 2 covers, triangle, drying oven. 

Note. — Parts of this experiment may be assigned to sections or individ¬ 
uals. To save time, a may be omitted and the experiment started with b ; 
see directions in b. This experiment may be deferred until § 299 in the 
author’s Practical Chemistry is studied. 

As in previous experiments, copy first the forms of Record ; enter 
the weights as soon as weighings are made. 

a. Moisture. — Weigh a clean, dry porcelain crucible and cover 
accurately on the balance. Remove the crucible from the balance 
pan, and slip about 2 gm. of the powdered coal into the crucible, 
taking care not to leave any dust on the edges or sides of the crucible. 
Weigh (with the cover). 

Put the crucible, uncovered, in an oven and heat for about an hour 
to 105 ° C. ( 104 - 107 ). Cool, and weigh with the cover. The loss 
in weight is the weight of the moisture. Save the crucible and con¬ 
tents for b. Calculate the per cent of moisture and enter it in 
Record —I. 


Record — I 


Weight of crucible, cover, and coal before heating . . . gm. 

Weight of crucible and cover..gm. 

Weight of coal. gm. 

Weight of crucible, cover, and coal before heating . . . gm. 

Weight of crucible, cover, and coal after heating .... _gm. 

Weight of moisture. gm. 

Per cent of moisture. per cent 


b. Volatile Matter. — If a has been done, use the crucible and 
contents. If a was omitted or is being done, start b with a new por¬ 
tion of coal. Enter the weights in Record — II. The loss in this 
case is the total volatile matter (that is, other volatile matter 
besides moisture). 









io8 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Place the covered crucible on a triangle which rests on a ring at¬ 
tached to an iron stand (Fig. 71). Heat gently at first, and then 
intensely for eight minutes, or for two or three minutes after the gases 
cease to burn between the crucible and cover. Cool the crucible 
slowly, and weigh (with the cover). The loss in weight is the vola¬ 
tile matter (combustible, if the crucible from a was used, total, if a 
new portion was used). Save the crucible and contents for c. Cal¬ 
culate the per cent of total volatile matter (and if a was done, the 
per cent .of combustible volatile matter) and enter in the proper 
place in Record — II. 


Record — II 


Weight of crucible, cover, and coal before heating . . . gm. 

Weight of crucible and cover.. 

Weight of coal.. & m - 

Weight of crucible, cover, and coal before heating . . . gm. 

Weight of crucible, cover, and contents after heating . . gm. 

Weight of volatile matter. S m - 

Per cent of volatile matter. P er cent 


c. Fixed carbon and ash. — If the crucible 
and contents from b are used, proceed at once 
to heat the uncovered crucible as in the next 
paragraph. If b was not done or the crucible 
is not available, start with a new portion as in a; 
heat the covered crucible containing the new 
portion of coal gently until most of the volatile 
matter has been expelled. Then remove the 
cover and proceed as in the next paragraph. 
Enter the weights in the proper places in 
Record — III. 

Incline the uncovered crucible slightly (Fig. 
72), heat gently at first and then intensely un¬ 
til all the carbon has been burned; if any car¬ 
bon remains on the inside of the cover, burn it 
* t us ' f or determin- °ff very carefully. Cool and weigh the covered 
ing the volatile crucible. The final weight of the substance in 
matter in coal the crucible is the weight of the ash. Calcu¬ 

late the per cent of ash. Calculate also the per 
cent of fixed carbon, utilizing the results in a and b for this calcula¬ 
tion and enter in Record — III. 



"FTn i t — Annara- 

















FUELS — ILLUMINATING GAS — FLAME 


109 


Record — III 


Weight of crucible, cover, and coal before heating ... gm. 

Weight of crucible and cover.. .gm. 

Weight of coal. gm. 

Weight of crucible, cover, and ash. I gm. II . . . gm. 

Weight of crucible and cover. gm. 

Weight of ash. gm. 

Per cent of ash. per cent 

Weight of coal. gm. 

Weight of volatile matter (total). gm. 

Weight of fixed carbon and ash. gm. 

Weight of ash. gm. 

Weight of fixed carbon. gm. 

Per cent of fixed carbon. per cent 


Experiment 126 — Properties of Gasolene 


O-csl 


Apparatus. — Hydrometer (specific gravity — direct reading) for liquids 
lighter than water, tall jar, medicine dropper, bottle fitted with cork. 

Caution. — Gasolene vapor catches fire 
quickly. Keep all flames away except as the 
experiment requires. 

a. Pour a few drops of gasolene into an 
evaporating dish. Note the odor. Cautiously 
bring a Bunsen flame near the surface of the 
liquid. Observe and state the result. 

b. Put a few drops of gasolene on a glass 
plate and note the result. Is gasolene vola¬ 
tile? Very volatile? 

c. Warm a 250 cc. bottle. Drop in (from 
a medicine dropper or a pointed glass tube) 
two or three drops of gasolene. Insert the cork 
and fill the bottle with vapor by rolling and 
shaking it. Uncork it, and hold a blazing joss 
stick at the mouth for an instant. Note the 
result. If the result is not striking, repeat with five or six drops of 
gasolene. State the result. Does gasolene explode? What does 
explode ? 

d. Determine the specific gravity of one or more samples of gaso¬ 
lene with the hydrometer (Fig. 73) as in Exp. 38. 


Fig. 72. — Apparatus 
for determining the 
fixed carbon in coal 
























no EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 127 — Properties of Kerosene 


Apparatus. — As in Fig. 74, thermometer. 


Compare the cor- 


a, b, c, d. Proceed as in Exp. 126 a, b, c, d. 
responding results of each experiment. 

e. Determine the flashing point of kerosene 
with the apparatus shown in Fig. 74. Fill the 
large beaker nearly full of water. Suspend the 
small beaker in the water by winding a copper wire 
around the top and twisting the ends of the wire 
around the large beaker just below the rim. Stand 
the large beaker on a gauze-covered ring or a piece 
of asbestos board. Fill the small beaker nearly 
full of kerosene. Clamp the thermometer so that 
the bulb is submerged in the kerosene. 

Heat the water gently and at intervals slowly 
pass a lighted match or a blazing joss stick about 
half an inch above the surface of the kerosene; 
when the vapor catches fire and a flash passes down 
to the surface of the kerosene, read and record the 
temperature. Let the water cool somewhat, and 
repeat the test. 

The lowest temperature at which the flame, 




^===b 


Fig. 73. — Ap- 
paratus for 
finding the 


specific grav- cause d by the burning vapor, passes completely 
ity of gasolene over the surface may be accepted as the flashing 
point of kerosene. 


Note. — The legal flashing point of commercial 
kerosene varies, but in most states it is about 44 0 C. 

Experiment 128 — The Principle of the 
Davy Safety Lamp 

a. Press a ,wire gauze down upon a Bunsen 
flame. Where is the flame? Remove the 
gauze, let it cool (or use another gauze), lower 
it upon the flame, and hold a lighted match 
just above the gauze. Now where is the 
flame? 

b. Extinguish the flame. Turn the gas on 
full, hold the gauze in the escaping gas, about 
15 cm. (6 in.) above the top of the burner, 
and thrust a lighted match into the gas above 



Fig. 74.;—Apparatus 
for finding the flash¬ 
ing point of kerosene 




















FUELS — ILLUMINATING GAS — FLAME 


hi 


the gauze. Move the gauze slowly back and forth. Where is the 
flame? Lower the gauze slowly and describe the final result. 

c. Hold the gauze in the flame in one position for a minute or two. 
Where is the flame at the end of this time? Why? 

Experiment 123 — Illuminating (Coal) Gas 

Materials. — Soft coal, litmus paper, lead nitrate solution. 

Apparatus. — As in Fig. 75. 

Fill the test tube two-thirds full of coarsely powdered soft coal, 
insert the stopper with its tube, and clamp 
the test tube carefully to the iron stand as 
shown in Fig. 75. - Heat the whole tube 
gently at first, gradually increase the heat, 
and finally heat intensely the part contain¬ 
ing the coal. 

a. As soon as the gas begins to escape, 
hold at the end of th£ tube a piece of fil¬ 
ter paper which has been moistened with 
lead nitrate solution; observe the effect 
upon the paper. The discoloration is 
caused by lead sulphide which is produced 
by the interaction of lead nitrate and the 
sulphides in the liberated gas. 

b. Lay a piece of wet red litmus paper 
on the end of the tube and continue to heat intensely; wet the 
paper, if it dries. Observe any change in the color of the litmus pa¬ 
per. To what class of compounds in the gas is the change due? 

c. Heat intensely, and light the gas at the end of the tube. Ob¬ 
serve and describe the flame. 

d. Discontinue heating, let the apparatus cool somewhat, dis¬ 
connect, and break open the test tube. Examine the contents. 
State the properties of both solid and liquid products; what is the 
name of each ? 



Experiment 130 — Testing Illuminating Gas 

Materials. — Solutions of calcium hydroxide, lead nitrate, potassium 
permanganate (very dilute). 

a. Test samples of illuminating gas for carbon dioxide, sulphides 
(Exp. 129 a), and ammonia. State the results. 












112 EXPERIMENTS IN PRACTICAL CHEMISTRY 


b. Suggest a test for moisture. Submit the details to the Teacher, 
before proceeding. 

c. Fill a bottle with illuminating gas as follows: Invert a bottle 
over a Bunsen burner (not lighted), turn on the gas and slowly dis¬ 
place the air with illuminating gas. When the bottle is full, turn off 
the gas, stand the bottle upright, quickly pour in about 5 cc. of very 
dilute (faint pink) potassium permanganate solution, cover with 
the hand, and shake well. Note the change in the color of the liquid. 
The change is caused by the illuminants (ethylene, etc.). 

Experiment 131 — Illuminating Gas Flame 

Materials. — Calcium hydroxide solution. 

Apparatus. — Gas burner (Fig. 76) or tip, glass tube. 

a. Examine a gas burner tip, noting especially the slit. 

b. If an ordinary gas burner is not available, attach the tip to a 
rubber tube and slip the tube over the top (or just inside) of a Bunsen 

burner. Light the# gas. Note the yellow 
and black parts. Turn off the gas slowly 
until the flame is very small and note the 
change in the size of the parts, and finally 
the black and the blue parts. Turn on 
the gas slowly and note the change in the 
size of the parts. Describe these changes. 
(See Fig. 76.) 

c. Hold a glass tube in the upper part of 
the yellow flame. Note the deposit on 
the tube. What is it ? Where did it come 
from? Lower the flame and hold a cold 
dry bottle low down almost upon the flame. 

Is a deposit formed? If so, what is 
it and why was it formed? 

d. Hold a cold dry bottle mouth down¬ 
ward just over the flame. What is the deposit inside the bottle? 
Pour about 10 cc. of calcium hydroxide solution into the bottle, 
and shake. Describe and explain the result. What are the two 
products of the combustion of illuminating gas? 

Experiment 132 — Candle Flame 

Materials. — Candle, piece of stiff paper, calcium hydroxide solution, 
lead pencil, copper wire (15 cm. or 6 in. long). 






FUELS — ILLUMINATING GAS — FLAME 


II3 

Stick a short candle to a block of wood by means of a little melted 
candle wax. 

a. Hold a cold, dry bottle over the lighted candle. What is the 
product seen inside the bottle ? What is its source ? Remove the 
bottle, pour in a little calcium 
hydroxide solution, and shake. 

Describe and explain the result. 

What are the two main products 
of a burning candle? 

b. Blow out the candle flame, 
and immediately hold a lighted 
match in the escaping smoke. 

Does the candle relight? Why? Fig - 77-— Effect of cooling a 
What is the general nature of this candle flame 

smoke ? How is it related to the candle wax ? 

c. Press a piece of stiff paper for an instant down upon the steady 
candle flame almost to the wick. Repeat several times with different 
parts of the paper. What do the marks on the paper show about 
the structure of the flame? 

d. Roll one end of the copper wire around a lead pencil to form 
a spiral about 2 cm. (or 1 in.) long. Press the spiral down slowly 
upon the candle flame (Fig. 77). Cool the wire and repeat. What 
is the result? Why? 

Optional Exercises. — 1. Draw a candle flame, showing the parts. 

2. Is there any essential difference between a candle and a gas or a lamp 
flame? 

3. Why do candles and lamps often smoke? 

Experiment 133 — Bunsen Burner and Bunsen Burner Flame 

Materials. — Powdered wood charcoal, pin, copper wire. 

a. Take apart a Bunsen burner and study the construction. Write 
a short description of the burner. Sketch the essential parts. 

b. Close the holes at the bottom of a lighted burner and hold a 
glass tube in the upper part of the yellow flame. Note the deposit. 
What is it? Where did it come from? Open the holes and move 
the tube up and down in tfie colorless Bunsen flame. What becomes 
of the deposit ? Why ? 

c. Dip a glass tube a short distance into some powdered wood char¬ 
coal, place the end containing the charcoal in one of the holes at the 
bottom of the lighted burner, and blow gently two or three times 
into the other end. Describe and explain the result. 








114 EXPERIMENTS IN PRACTICAL CHEMISTRY 


d. Open and close the holes of a lighted burner several times. De¬ 
scribe the result. Pinch the rubber tube to extinguish the flame, 
then light the gas at the holes. What change is produced in the 
flame? What is the object of the holes? 

e. Lay a match across the top of the tube of a lighted Bunsen 
burner. When the match begins to burn, remove and extinguish 
it. Note where it is charred, and explain the result. 

Press a piece of wire gauze down upon the flame. Describe and 
explain the appearance of the gauze (Fig. 78). 

Stick a pin through a match near the head, and suspend it across 
the burner (Fig. 79). Turn the gas on full and light it. What is 
the effect on the match? What does the whole of e show about the 
structure of the lower part of the Bunsen flame? Verify your answer 
by f. 

f. Hold one end of a glass tube (about 15 cm. or 6 in. long) in the 
Bunsen flame about 2 cm. (1 in.) from the top of the burner tube 



Fig. 78. — Studying 
the cones of a 
Bunsen flame 



k \ l 


Fig. 79. — Studying 
the lower part of 
a Bunsen flame 



M 

Fig. 80. ‘— Studying 
the inner cone of 
a Bunsen flame 


(Fig. 80). Hold a lighted match for an instant at the upper end 
of the tube; raise or lower the tube slightly (still keeping the end 
in the flame) and observe the result. What does the result show 
about the structure of the Bunsen flame? How does it verify e? 

g. Find the hottest part of the flame, when a full current of gas 
is burning, by holding a copper wire in the flame (Fig. 2). Meas¬ 
ure its distance, approximately, from the top of the burner tube. 

h. Examine an imperfect Bunsen burner flame — one which shows 
the outlines of the inner part. What is the general shape of each 
main part? Draw a vertical and a cross section. 

i. Using the same burner as in h, lower the flame gradually until 











FUELS — ILLUMINATING GAS — FLAME 


115 


it strikes back. Now observe the place where the gas burns, 
the odor. Feel cautiously of the tube and describe the result. 


Note 


1 / 


Fig. 81. — Blow¬ 
pipe tube 


Experiment 134 — Reduction and Oxidation with the Blowpipe 

Materials. — Charcoal, lead oxide, sodium carbonate, sodium sulphate, 
powdered wood charcoal, silver coin, zinc, lead, tin. 

Apparatus. — Blowpipe, blowpipe tube. 

Slip the blowpipe tube (Fig. 81) into the burner tube. Light the 
gas and lower the flame until it is about 4 cm. 

(1.5 in.) high. Rest the tip of the blowpipe (Fig. 

82) on the top of the blowpipe tube, placing the tip 
just within the flame. Put the other end of the 
blowpipe between the lips, puff out the cheeks, 
inhale through the nose, and exhale into the blow¬ 
pipe, using the cheeks somewhat as bellows. Do 
not blow in puffs, but produce a continuous flow 
of air through the blowpipe (Fig. 83). The flame 
should be an inner blue cone surrounded by an 
outer and almost invisible cone (Fig. 84). 

__ A. Reduction. — a. Make 

—^ a cavity in one end of the flat 
side of a piece of charcoal. 
Fill it with a mixture of equal 
Fig. 82. Blowpipe parts of powdered sodium 

carbonate and lead oxide, and heat the mixture in the reducing 
flame (B in Fig. 84). In a short time 
bright, silvery globules should appear on the 
charcoal. Let the mass cool, and pick out 
the largest globules. Put one or two in a 
mortar, and strike with a pestle. Are they 
soft or hard? Malleable or brittle? How 
do the proper¬ 
ties compare with 
A £ those of metallic 

Fig. 84.— Blowpipe flame lead? What has 
— A (oxidizing) and B become of the 
(reducing). The flame is oxygen? 
coming out of the upper b. Grind to- 
end of the blowpipe tube gether in a mor¬ 
tar a little sodium sulphate and powdered 


r 



Fig. 83. — Using the 
blowpipe 







n6 EXPERIMENTS IN PRACTICAL CHEMISTRY 


wood charcoal, adding at intervals just enough water to hold 
the mass together. Heat some of this paste in the reducing flame 
as in a. Scrape the mass into a test tube, boil in a little water, and 
put a drop of the solution on a bright silver coin. If a dark brown 
stain is produced, it is evidence of the formation of silver sulphide. 
Repeat, if no such stain is produced. The silver sulphide is formed 
by the interaction of the silver and sodium sulphide. Explain how 
the experiment illustrates reduction. 

B. Oxidation. — a. Heat a small piece of zinc on charcoal in the 
oxidizing flame (A in Fig. 84). Direct the flame across the zinc so 
that most of the product will form a coating on the charcoal. What 
is the product? Observe the color of the coating on the charcoal 
when both hot and cold. Record the result. 

b. Heat a piece of lead as in a. Observe the color of the coatings 
(hot and cold). Record the result. 

c. Optional. Heat a small piece of tin in the oxidizing flame. Ob¬ 
serve and record as in b. 

Optional Exercises. — 1. Name the products formed in B. 

2. Sketch a flame showing the oxidizing and reducing parts. 

Experiment 135 — Testing for Metals and Non-metals 

Materials. — Compounds of zinc, lead, and tin, insoluble sulphates ( e.g. 
of calcium, barium, lead), charcoal. 

Obtain “ unknowns ” and apply (1) the blowpipe or the flame 
test for the metal, (2) the blowpipe test for an insoluble sulphate, 
and (3) if necessary other tests, e.g. for chloride, sulphate, carbonate, 
nitrate. State each result. 

Give the name and formula of each compound. 


OTHER CARBON COMPOUNDS 

(Practical Chemistry, pp. 289-305, §§ 339-372) 

Experiment 136 — Sucrose (Cane Sugar) and Dextrose 

a. Proceed as in Exp. 114 e. 

b. Proceed as in a, using dextrose instead of sucrose. Compare 
the results. 

c. Add 10 cc. of Fehling’s solution (see App. § 6, List G) to 5 cc. 
of dextrose solution, and heat to the boiling point. Note the result. 
The precipitate is cuprous oxide. Describe it. 



OTHER CARBON COMPOUNDS 


117 

d. Repeat c, using cane sugar solution instead of glucose. Do 
not boil the mixed solutions. State the result. Compare with a. 

e. Apply Fehling’s test for dextrose (and similar sugars) to cheap 
candy, maple sugar, molasses, table sirups, jelly, jam, etc. Prepare 
and use clear solutions. State each result. 

Experiment 137 — Properties of Starch 

Materials. — Starch, Fehling’s solution, iodine solution. 

Prepare a starch mixture by boiling about 1 gm. of powdered 
starch for a few minutes in 50 cc. of water; stir or agitate the mix¬ 
ture during the boiling. Make three tests with the starch mixture. 

(1) Pour half of it into an evaporating dish which stands on a 
gauze-covered ring, add 1 cc. of concentrated sulphuric acid, mix 
well, and boil for at least ten minutes; add water occasionally to 
replace that lost by evaporation. Meanwhile proceed with (2). 

As soon as the mixture (in (1)) has been boiled at least ten min¬ 
utes, take out a little, add sodium hydroxide solution to alkaline 
reaction and apply Fehling’s test. Note the result. Continue the 
heating for ten or more minutes, and test again. State the final re¬ 
sult. 

(2) Dilute half of the rest of the original starch mixture with water 
and test it with Fehling’s solution. Observe and state the final re¬ 
sult. Compare with (1). 

(3) Add a drop or two of very dilute iodine solution to the rest of 
the starch mixture. Observe the color. (This test for starch is 
delicate, and dilute mixtures should be used.) 

Experiment 138 — Detection of Starch by Iodine 

Materials. — Dilute solution of iodine; potato, rice, bread, and sub¬ 
stances enumerated in b. 

a. Test potato, rice, and bread for starch by moistening each sep¬ 
arately with water, and then adding a drop or two of very dilute iodine 
solution. State the result in each case. 

b. Proceed as in a, using substances not positively known to con¬ 
tain starch, e.g. baking powder, leaves of different kinds of trees, roots 
of vegetables, popped corn, straw, and various kinds of food. State 
each result. 

Experiment 139 — Properties of Ethyl Alcohol 

Materials. — Ethyl alcohol, camphor, shellac, rosin, iodine, ether, carbon 
disulphide, carbon tetrachloride. 


n8 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Apparatus. — Tall jar, hydrometer for light liquids (as in Exp. 126). 

a. Drop a little ethyl alcohol on a glass plate, and watch it evapo¬ 
rate. Does it evaporate more rapidly than water? 

b. Weigh a measured quantity (about 25 cc.) of alcohol in a grad¬ 
uated cylinder and calculate its specific gravity. (See Exp. 114 a.) 

c. Determine the specific gravity of alcohol with the hydrometer. 
State the result. (See Exps. 114 a and 126 d.) 

d. Try the solvent power of alcohol by adding powdered sub¬ 
stances to 5 cc. in separate test tubes, e.g. camphor, powdered shellac, 
rosin, or iodine. Describe each result. Add water to each solution. 
Describe and explain the result. 

e. Proceed as in d, using liquids, e.g. water, ether (care!), carbon 
disulphide (care!), carbon tetrachloride. State each result. 

f. Burn a little alcohol in a porcelain dish and observe the proper¬ 
ties of the flame, e.g. color, heat. What are the products of com¬ 
bustion ? 

Experiment 140 — Tests for Ethyl Alcohol 

a. Proceed as in Exp. 142 a. 

b. To 5 cc. of ethyl alcohol add a crystal or two of iodine and just 
enough sodium hydroxide solution to dissolve and decolorize the 
iodine. Warm gently several minutes and then cool. Note the 
odor of the yellow product. It is iodoform and its formation is a 
test for alcohol. 

Experiment 141 — Properties of Acetic Acid 

Materials. — Acetic acid, magnesium ribbon. 

a. Put 5 cc. of acetic acid in a test tube. Note the odor and taste 
(cautiously). Warm a little in a test tube, and smell (cautiously). 
Describe the odor. Is acetic acid volatile? Test with litmus paper, 
and describe the result. 

b. Prepare, or obtain, a solution of 5 cc. of acetic acid in 15 cc. 
of water and a similar solution of sulphuric acid and water. Drop 
a short piece of magnesium ribbon into each and note the result. In 
which acid is the action faster? Is acetic acid a weak or a strong 
acid? 


Experiment 142 — Test for Acetic Acid and Acetates 

Materials. — Concentrated sulphuric acid, acetic acid, ethyl alcohol, 
sodium acetate solution. 


OTHER CARBON COMPOUNDS 


ii 9 

a. Cautiously add a few drops of concentrated sulphuric acid to 
a mixture of 5 cc. each of acetic acid and ethyl alcohol. Shake the 
mixture and warm gently. Note the odor. The pleasant, fruitlike 
odor is due to ethyl acetate. 

b. Proceed as in a, using sodium acetate solution. 

Experiment 143 — Properties of Vinegar 

Materials. — Vinegar, solutions for a, sodium cobaltinitrite solution (for 

b (2)). 

a. Show that vinegar contains acetic acid. 

b. Evaporate 15 cc. of vinegar to dryness on a water bath and 
note the residue. Stand the dish on a gauze-covered ring and heat 
gently. Note the ash. 

Test the ash for (1) a carbonate and (2) potassium. (1) Add 
dilute hydrochloric acid to the residue, and note the effervescence. 
Warm gently to expel the gas, and filter. (2) To the filtrate from 
(1) add 5 to 10 cc. of sodium cobaltinitrite solution. The yellow 
precipitate is a test for potassium (compare Exp. 182 b). 

Experiment 144 — Preparation of Soap 

Materials. — Sodium hydroxide, lard, salt. 

a. Dissolve 10 gm. of sodium hydroxide in 75 cc. of water, add 
30 gm. of lard, and boil the mixture in a porcelain (or metal) dish 
for an hour or more; add water occasionally to replace that lost by 
evaporation. Then add 20 gm. of fine salt in small portions. Stir 
constantly during the addition of the salt. Let the mass cool, and 
remove the cake of soap. 

b. Optional for Class or Teacher. Prepare soap by the method 
given on a can of commercial “ lye.” 

Experiment 145 — Properties of Soap 

Materials. — Soap, sulphuric acid; calcium sulphate, magnesium sul¬ 
phate, and acid calcium carbonate solutions for e. 

a. Leave soap shavings exposed to the air for several days. What 
does the result show about the presence of water in the soap ? 

b. Test the soap made in Exp. 144 with wet litmus paper. State 
the result. Test other samples and compare. 

Put a few drops of phenol-phthalein solution (alcoholic) on samples 
of dry soap. State the result. This is a test for “ free alkali.” 

c. Prepare 25 cc. of a solution of the soap made in Exp. 144 


120 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Warm it and examine the surface for fat (film or globules). Is fat 
detected? Why? 

d. Add 20 cc. of dilute sulphuric acid to io cc. of soap solution. 
Note the result. The precipitate is a mixture of palmitic and stearic 
acids. Describe it. 

e. Optional. See Exp. 191. 

Experiment 146 — Carbon Tetrachloride 

Materials. — Carbon tetrachloride, joss stick. 

Apparatus. — Iron crucible, pyrene fire extinguisher (for b). 

a. Heat the bottom of an iron crucible (or metal pan), drop in 
some carbon tetrachloride, and hold a blazing joss stick or a piece 
of burning paper in the vapor. Describe the result. 

b. Optional. Examine and describe a pyrene fire extinguisher. 


FOOD AND NUTRITION 

(Practical Chemistry, pp. 307-314, §§ 373-382) 

Experiment 147 — Testing for Nutrients in Food 

Materials. — Foods; Molisch’s, iodine, Fehling’s and sodium hydroxide 
solutions; gasolene, concentrated nitric acid, soda lime (for d ( 1 ) ), 
very dilute copper sulphate solution. 

Apply tests for carbohydrate, fat, and protein to various foods 
from the Table in §§ 377 and 381 of the author’s Practical Chemistry. 

a. Carbohydrate. — Apply the Molisch test. To 5 cc. of a clear 
dilute solution of the carbohydrate (or food), add 2 cc. of Molisch’s 
solution, and shake. Incline the test tube and carefully pour down 
the inside 5 cc. of concentrated sulphuric acid so that two layers will 
form. At the contact zone a red-violet color will appear slowly. 
State the result. 

b. Carbohydrate. — Test for starch (Iodine Test — Exps. 137 b 
(3), 138) and sugar (Fehling’s Test —Exp. 136 c). State each re¬ 
sult. 

c. Fat. — Grind the sample with gasolene (care!) in a mortar, I 
pour off the gasolene into an evaporating dish (filter, if not clear),- 
let it evaporate, and examine the residue. Rub a little between the 
fingers. Burn a little on the end of a glass rod. State each result. 

d. Protein. — (Note. — Use two or more of these tests.) (1) Pro¬ 
ceed as in Exp. 54 a. 





FOOD AND NUTRITION 


I 2 I 


(2) Grind the sample with 20 cc. of water in a mortar, pour off 
the water (filter, if not clear). To about 5 cc. of the dilute extract 
add an equal volume of sodium hydroxide solution and shake well. 
Then add drop by drop a very dilute copper sulphate solution. A 
violet color is produced. 

(3) To 5 cc. of the extract from (2) add an equal volume of con¬ 
centrated nitric acid. Heat gently until a yellow precipitate or a 
yellow solution is obtained. Cool in running water and add an ex¬ 
cess of sodium hydroxide solution. An orange color is produced. 

(4) To 5 cc. of the extract from (2) add concentrated nitric acid 
slowly, pouring the acid down the inside of the tube so the two solu¬ 
tions will not mix. A white cloudy precipitate is formed at the sur¬ 
face of the two liquids. 

Experiment 148 — Testing for Water in Food 

a. Proceed as in Exp. 25 a, using samples from the Table in § 377 
of the author’s Practical Chemistry. State each result. 

Experiment 149 — Testing for Mineral Matter in Food 

Heat a sample of the food in an evaporating dish or crucible, or on 
a piece of porcelain, in the hood, until the residue is white or gray. 
This is the mineral matter. If the food, e.g. beans, cheese, or peanuts, 
contains considerable mineral matter, tests may be applied to the 
residue. See Exp. 153 e for phosphorus, Exp. 153 h for calcium, 
and Exps. 143 b (2) and 182 b for potassium. 

Experiment 150 — Testing Bread 

a, b, c. Carbohydrate, Fat, Protein. — Proceed as in Exp. 147 
b, c, d, using samples of bread. State each result. 

d. Water. — ( 1 ) Proceed as in Exp. 25 a, using bread. 

(2) Optional. Weigh a porcelain dish, put in a piece of fresh 
bread about 5X5X1 cm., and weigh again. Heat the dish gently 
in an oven (not above 105° C.) for several hours or let it stand for 
several days in a desiccator containing concentrated sulphuric acid. 
Weigh again. What weight of water was lost? What per cent? 

e. Mineral matter. — Proceed as in Exp. 149, using bread. State 
the result. 

Experiment 151 — Testing Butter and Substitutes 

a. Put a small lump of butter in an evaporating dish, heat gently 
with a small flame, and note the result. 


122 EXPERIMENTS IN PRACTICAL CHEMISTRY 


b. Proceed as in a, using separately samples of butter substitutes 
Note the result and compare with a. 

Experiment 152 — Testing Milk 

Materials. — Milk, acetic acid, sodium hydroxide, dilute copper sulphate 
solution, junket tablet, gasolene; ammonium oxalate and ammonium 
molybdate solutions (for d). 

Apparatus. — Babcock apparatus — Fig. 85 — (for c (2)). 

a. Water and solids. — Clean and dry an evaporating dish. Weigh 
it together with a glass rod (about 8 cm. long) on the balance (or 
good scales). Record the weight. Pour about 25 cc. of well-mixed 
milk into the dish and weigh again. Record the weight. The dif¬ 
ference between these weights is the weight of the milk. Stand the 
dish on a water bath and evaporate to dryness, stirring occasionally 
to hasten evaporation. Meanwhile do b, etc. 

When the residue is dry, let the dish cool, wipe it dry, and weigh. 
The decrease in weight is due to the loss of water. Save the residue 
for c. From the weight of the milk taken and the weight of the 
residue, calculate the per cent of (1) water and (2) solids in the 
milk. (Milk contains about 88 per cent of water. Unless the resi¬ 
due is dry, the result will be only approximate.) 

b. Protein. — (1) Boil about 50 cc. of milk in an evaporating (or 
other) dish. Note the formation of a scum. Remove this scum 
with a glass rod to a test tube, collecting several portions, and test it 
as in Exp. 147 d (2) (or another test). 

(2) Add 3 or 4 drops of acetic acid to 10 cc. of milk in a test tube, 
and shake. The curdy precipitate is casein. Filter, and test the 
solid for protein as in (1). Test the filtrate for albumin (a kind of 
protein) by boiling; the heat coagulates the albumin into white 
flakes. 

(3) Add^a small fragment of a junket tablet to 10 cc. of warm 
milk. Separate and test as in (2). 

c. Fat. — (1) To the residue from a add 10 cc. of gasolene (care!) 
and mix well. Pour off the gasolene into a beaker or a dish and let 
it evaporate. Save the dish and contents for d. Examine the solid 
from the gasolene extract. Rub a little between the fingers, and 
burn a little on the end of a glass rod. Is fat detected? 

(2) Optional or Demonstration Experiment. The Babcock test. 
Shake the sample of milk, measure 17.6 cc. into the special milk grad¬ 
uate (Fig. 85 A), and pour it carefully into the test bottle (Fig. 85 B). 
If a pipette (Fig. 85 C), instead of a graduate, is used, fill the pipette 


FOOD AND NUTRITION 


123 


as follows: Put the lower end well into the milk and the other end 
into the mouth; suck out the air until the milk rises above the 17.6 cc. 
mark on the stem, remove the pipette from the mouth and quickly 



Fig. 85.— Babcock apparatus for testing milk — A, milk graduate; B , 
test bottle; C, pipette; D, acid graduate; E, centrifugal machine 

cover the end with the finger; move the finger a little and let milk 
run out slowly until it reaches the 17.6 cc. mark. 

Next measure 17.5 cc. of concentrated sulphuric acid into the spe¬ 
cial acid graduate (Fig. 85 D ). Pour the acid carefully in small por¬ 
tions into the test bottle. Shake carefully after each addition. This 
operation dissolves the curd ( i.e . the casein) and facilitates the sep¬ 
aration of the fat. 

Label the bottle and put it in the centrifugal machine (Fig. 85 E ) 
together with three other bottles filled similarly with milk and acid, 
or with water (if only one test is being made). Whirl the machine 
rapidly and uniformly for five minutes; the melted fat will rise and 
collect on the surface of the liquid. Add enough hot water to fill 
the larger portion of the bottle, and whirl for two more minutes. 
Then add hot water carefully until the water is just below the top 
graduation on the stem (not above the graduation), and whirl again 
for two minutes. 

Remove the bottle from the machine and stand it in a dish con¬ 
taining water at 6o° C. In a minute or two, remove the bottle and 
read the volume of fat, taking care to read from the top of the upper 
meniscus (curved surface of the fat) to the bottom of the lower menis¬ 
cus. The difference between the two readings is the per cent of fat 





















124 EXPERIMENTS IN PRACTICAL CHEMISTRY 


in the milk. Report the per cent to the Teacher before throwing 
away the contents of the bottle. If the result is accepted, pour the 
liquid into a waste jar and wash the bottle clean with hot water. 

d. Mineral matter. — If the dish and contents (from which the 
fat was extracted) from c (i) is available, use it. If not, evaporate 
io cc. of milk to dryness and use the residue. Heat the dish and 
contents in the hood until the residue is white or gray. Dissolve 
this mineral matter in water and test portions for calcium and a 
phosphate (as in Exp. 153 h, e). State the results. What component 
of milk contains most of the mineral matter? 

Experiment 153 — Testing Baking Powders 

Materials. — Baking powder (tartrate, phosphate, alum), barium hy¬ 
droxide, vinegar, sour milk, lemon juice, solutions of iodine, silver ni¬ 
trate, ammonium chloride, sodium hydroxide, and ammonium oxalate. 

Note. — Different varieties of baking powder may be tested by individ¬ 
uals or sections, and the results compared. 

a. Carbonates. — (1) Put a little baking powder in a test tube, 
add a few drops of dilute hydrochloric acid, and test the escaping 
gas with a tube which has been dipped into barium hydroxide solu¬ 
tion. State the result. 

(2) Put 2 gm. of baking powder in a test tube, add 15 to 20 cc. of 
water, and shake well. Let the action continue a short time, and 
then test the solution as in (1). State the result. 

(3) Add sour substances, e.g. vinegar, sour milk, lemon juice, 
separately to a little baking powder, and state the result. 

b. Starch.—Apply the iodine test for starch to a little baking 
powder mixed with water. See Exp. 137 (3). State the result. 

c. Tartrates. — Prepare a cold solution of baking powder by shak¬ 
ing about 10 gm. of the substance with 50 cc. of water and stirring 
until all the gas is liberated. Filter, if not clear, and use the clear 
solution in this and succeeding experiments. (1) Clean a test tube 
by boiling sodium hydroxide solution in it and then washing thor¬ 
oughly with water. Put 10 cc. of silver nitrate solution in the cleaned 
test tube, and add ammonium hydroxide slowly until the precipitate 
at first formed redissolves, taking care to mix the solutions. Add 
10 cc. of the baking powder solution and warm gently. Tartrates, 
if present, will reduce the silver compound to silver, which will coat 
the inside of the test tube. (2) Put about 5 cc. of the solution from 
c in an evaporating dish, add a few drops of concentrated sulphuric 



SILICON 


125 


acid, and heat gently. Tartrates, if present, will char and smell 
like burnt sugar. 

d. Sulphates. — To 5 cc. of the baking powder solution (prepared 
in c) add dilute hydrochloric acid to acid reaction and boil; then 
test with barium chloride solution. State the result. 

e. Phosphates. — Warm 5 cc. of the baking powder solution, 
acidify with concentrated nitric acid, and add 5 cc. of ammonium 
molybdate solution. A yellow precipitate indicates phosphates. 
State the result. 

f. Ammonium salts. — Boil 5 cc. of the baking powder solution 
with an equal volume of sodium hydroxide solution. The presence of 
ammonium salts is shown by the liberation of ammonia gas, which 
can be detected by its odor. State the result. 

g. Aluminium salts. — Boil 5 cc. of the baking powder solution 
with 1 or 2 cc. of dilute hydrochloric acid, filter if not clear, and add 
10 cc. or more each of ammonium chloride and ammonium hydrox¬ 
ide to the filtrate. A whitish flocculent precipitate (aluminium hy¬ 
droxide) indicates aluminium salts. State the result. 

h. Calcium salts. — Boil 10 cc. of the baking powder solution 
with dilute hydrochloric acid (to remove the carbon dioxide), add 
ammonium hydroxide to alkaline reaction, filter, if not clear and 
then add ammonium oxalate solution. Calcium compounds produce 
a white precipitate (calcium oxalate). 


SILICON 

(Practical Chemistry, pp. 316-327, §§ 383-395) 

Experiment 154 — Preparation of Sodium Silicate 

Materials. — Powdered silicon dioxide, sodium carbonate. 

Apparatus. — Iron crucible. 

Mix thoroughly about 0.5 gm. of fine sand and 4 gm. of sodium 
carbonate and put the mixture in an iron crucible. Stand the cru¬ 
cible on a triangle (or in a small ring) and heat gently until the mass 
ceases to bubble. Then heat intensely for ten or fifteen minutes. 
Allow the crucible to cool somewhat, add 25 cc. of hot water, and heat 
until the water boils. When cold, filter, and evaporate the filtrate 
to about half its volume. This solution contains sodium silicate. 
Save it for Exp. 155. 

State the chemical changes by which silicon dioxide is transformed 
into sodium silicate. 


126 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 155 — Silicic Acid 

Materials. — Sodium silicate solution, hydrochloric acid. 

a. To the solution from Exp. 154 add dilute hydrochloric acid 
drop by drop, shaking constantly until a precipitate is formed. The 
precipitate is silicic acid. Describe it. 

b. Optional. Put 10 cc. of commercial sodium silicate solution 
in an evaporating dish, and add 10 to 15 cc. of dilute hydrochloric 
acid, stirring constantly. The jellylike precipitate is silicic acid. 
Rub some between the fingers and state the result. 

Stand the dish on a gauze-covered ring attached to an iron stand 
and evaporate the solution slowly to dryness in the hood. As the 
mass thickens, stir it with a glass rod. Toward the end add more 
hydrochloric acid and evaporate to complete dryness. Then heat 
intensely for five minutes. When the dish is cool, add about 50 cc. 
of water, stir well, and filter; wash the residue with water once or 
twice, dry it, remove as much as possible from the paper, and heat 
it carefully in an evaporating dish for about five minutes. Rub 
some between the fingers or across a glass plate. State the result. 
Collect some within the loop of a test wire and heat it intensely in 
the flame for several minutes. State the result. What is this resi¬ 
due? 

State the chemical changes that occur in changing sodium silicate 
into the final residue. 

Experiment 156 — Testing for Silicon 

Materials. — Powdered calcium fluoride, sand, substances for b. 
Apparatus. — Lead dish, test wire. 

a. Put a little sand and calcium fluoride in a lead dish (see Fig. 86, 
Exp. 158), add enough concentrated sulphuric acid to moisten the 
mixture, and stir with a match. Dip the looped end of a test wire 
into water, inclose a film of water within the loop, and hold the loop 
at several points near the mixture in the dish until the water (in the 
loop) becomes white. If no change occurs, stir the mixture and 
hold the loop over the place where there is evidence of chemical action. 
State the result. What is the white substance in the loop? State 
in words the chemical changes that led to the formation of the white 
substance in the loop. Write the equations. 

b. Apply the test for silicon to several of these substances (omit¬ 
ting the sand): Powdered calcium fluoride, infusorial earth, pumice 
(powder), scouring soap, glass (small fragments), carborundum 


FLUORINE — BROMINE — IODINE 


127 


(powder), ash from coal, electro-silicon, glass wool, mineral wool, 
soil. State the result in each case. 

Experiment 157 — Carborundum 

Examine and describe carborundum. Try its hardness on glass, 
wood, and other solids, and state the result. Wind a test wire around 
a small lump, heat intensely for ten minutes, and state the result. 


FLUORINE — BROMINE — IODINE 


(Practical Chemistry, pp. 337-344, §§ 404-418) 


Experiment 158 — Etching with Hydrogen Fluoride 


Materials. — Paraffin, powdered calcium fluoride. 
Apparatus. — Lead dish, glass plate (see Fig. 86). 


Caution. — Do not inhale hydrogen fluoride. 

Warm a glass plate about cm. (4 in.) square by dipping 
it into hot wa- _ 



PMA€TE€AJL 


Fig. 


86. — Etching with hydrogen fluoride — lead uish 
(left), etched glass plate (right) 


ter or by mov¬ 
ing it slowly 
above a flame. 

Coat one sur¬ 
face uniformly 
with a thin 
layer of paraf¬ 
fin wax. Scratch letters, figures, or a diagram through the wax with 
a pin or pointed glass rod. The wax should be removed through to 
the glass, and the lines should be rather coarse. 

Put about 5 gm. of powdered calcium fluoride in a lead dish and 
add just enough concentrated sulphuric acid to form a thin paste 
(Fig. 86). Stir the mixture with a match. Place the glass, wax 
side down, upon the lead dish and let the whole stand in the hood for 


several hours. 

Remove the glass and scrape off the wax with a knife. The last 
portions can be removed by rubbing with a cloth moistened with 
hot water. Do not attempt to melt off the wax over the flame. Ex¬ 
amine and describe the glass (Fig. 86). 

State in words the essential chemical changes in this experiment. 
Write the equations. 

Note. —The lead dish should be cleaned in the hood by scraping the 
contents carefully into a waste jar and washing the whole dish with watei. 










128 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 159 — Preparation and Properties of Bromine 



Materials. — Potassium bromide, manganese dioxide, sulphuric acid. 
Apparatus. — As in Fig. 87 for b; bottle fitted with a cork. The large 
test tube has a one-hole rubber stopper to which is fitted the bent glass 
tube; the total length of the glass tube is about 30 cm. (12 in.). 

Caution. — Bromine is a corrosive liquid, which readily forms a suffo¬ 
cating vapor. Perform all experiments with bromine in the hood. 

a. Short method. — Put a little powdered potassium bromide 
and twice the bulk of manganese dioxide in a test tube. Add 5 cc. of 
dilute sulphuric acid and mix well. At¬ 
tach a test tube holder and heat gently. 
Bromine vapor is evolved. Note the color 
and very cautiously the odor. If any of 
the vapor condenses on the inside of the 
test tube, describe the liquid. (See Note 
below.) 

b. Long method. — Put about 3 gm. of 
potassium bromide in a large test tube, 
and add 5 gm. of manganese dioxide ; shake 
well, and add 10 cc. of dilute sulphuric 
acid. Insert the stopper and its tube 
(Fig. 87), attach the test tube holder, and 
warm gently. Bromine vapor soon ap¬ 
pears in the test tube and, if the heat is sufficient, some vapor will 
escape from the delivery tube. Note the color and very cautiously 
the odor. Is the vapor heavier or lighter than air? 

Heat to such a temperature that the vapor will condense and col¬ 
lect in the bend A of the delivery tube. When no further boiling 
produces bromine vapor in the test tube, transfer the bromine from 
the delivery tube into a bottle half full of water by holding the end 
of the delivery tube over the mouth of the bottle and heating the test 
tube slightly; the expanding gases will force the liquid bromine out 
of the bend into the bottle. 

Observe and record the physical properties of this bromine, espe¬ 
cially the color, solubility in water, specific gravity, volatility, and 
physical state. As soon as these observations have been made, cork 
the bottle tightly and shake it vigorously. Observe the result, and 
draw a conclusion about the solubility of bromine in water. 

Note. — Wash the delivery tube free from bromine, taking care to get 
none on the hands. Throw the contents of the test tube into a waste jar 
in the hood and wash the tube. 


Fig. 87. — Apparatus for 
preparing bromine 






FLUORINE — BROMINE — IODINE 


129 


Experiment 160 — Tests for Bromides 

Materials. — Potassium bromide, silver nitrate solution, carbon tetra¬ 
chloride. 

a. Add a little concentrated sulphuric acid to a little potassium 
bromide in a test tube; warm slightly, if the action is not marked. 
Observe the result, especially the color of the liquid or of the vapor 
just above the liquid. What element does the color suggest ? 

b. Dissolve a crystal of potassium bromide in a test tube half full 
of water, add a little silver nitrate solution, and shake. Observe 
the properties of the precipitate, especially the color and texture. 
Determine the solubility by warming a little of the precipitate in 
ammonium hydroxide. State the result. Compare silver bromide 
and silver chloride (Exp. 65 III b). 

c. To a solution of a bromide, add a little chlorine water and a 
few drops of carbon tetrachloride, and shake. The carbon tetra¬ 
chloride will be colored yellow or brown by the liberated bromine. 

Experiment 161 — Preparation and Properties of Iodine 

Materials. — Potassium iodide, manganese dioxide, concentrated sulphuric 
acid, cotton, alcohol, carbon tetrachloride, potassium iodide solution. 
Apparatus. — As in Fig. 88 (for b). 

Do a or b. a. Short method. — Proceed as in 
Experiment 159 a, using potassium iodide in place 
of potassium bromide. Note the color and (cau¬ 
tiously) the odor of the vapor, and the color of 
the sublimed iodine. 

b. Long method. — Grind together in a mortar 
about 3 gm. of potassium iodide and 5 gm. of man¬ 
ganese dioxide. Put the mixture in a test tube, add 
about 3 cc. of water, 5 cc. of concentrated sul¬ 
phuric acid, and mix well. Clamp the test tube 
vertically to an iron stand (Fig. 88). Close up the 
inner end (A in Fig. 88) of the stem of the funnel r 
with a small plug of cotton. Hold, or place, the 
funnel over the mouth of the test tube, and heat ^ ^ 
the test tube gently. The vapor of the liberated paratus for pre¬ 
iodine will fill the test tube, and crystals will form in paring iodine 

the upper part of the test tube and in the funnel. 

Continue to heat until enough iodine for several experiments collects 
in the funnel. Scrape the crystals into a dish. 












130 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Observe and record the color of the solid and of the vapor, and 
the odor (cautiously). 

Determine the volatility by putting a small piece in a bottle and 
exposing to the sunlight. 

Heat a crystal in a dry test tube, and invert the test tube when it 
is full of vapor. What does the result show about the density of 
iodine vapor? 

Touch a crystal with the finger. What color is the stain? 

Try the solubility separately in water, alcohol, carbon tetrachloride, 
and potassium iodide solution. What do these results show about 
the solubility of iodine ? 

Note. — If crystals are left, use them'in the next experiment. Preserve 
the iodine in a stoppered bottle, if not used at once. 

Experiment 162 — Tests for Free Iodine 

Materials. — Very dilute iodine solution, potassium iodide, carbon tetra¬ 
chloride, cold starch mixture. 

a. Add a few drops of carbon tetrachloride to a very dilute iodine 
solution. Shake well, and observe the color of the carbon tetra¬ 
chloride. 

b. Add 5 cc. of a cold starch mixture to a test tube nearly full of 
water, and then add a few drops of dilute iodine solution. Note the 
color. Pour about 5 cc. of the liquid into a test tube nearly full of 
water and shake. Note the color. 

Experiment 163 — Tests for Iodides 

Materials. — Potassium iodide, chlorine water, starch, carbon tetrachloride, 
silver nitrate solution. 

a. Add a few drops of carbon tetrachloride to a very dilute solution 
of potassium iodide. Then add several drops of chlorine water, 
and shake well. Note the color. 

b. Add 5 cc. of cold starch solution to 10 cc. of a very dilute solu¬ 
tion of potassium iodide. Add a few drops of chlorine water, and 
shake well. Observe and explain the result. 

c. To 10 cc. of potassium iodide solution, add a little silver nitrate 
solution, and shake. Observe the properties of the precipitate, es¬ 
pecially the color and texture. Test the solubility of a little of the 
precipitate in ammonium hydroxide, and state the result. Compare 
silver iodide with silver chloride and silver bromide (see Exps. 65 III b, 
160 b). 


PHOSPHATES — ARSENIC — ANTIMONY 


I3i 

Experiment 164 — Halogen Acids 

Proceed as in Exp. 64 a, b, d (omit c), using ( 1 ) potassium bromide 
and (2) potassium iodide in separate test tubes. 

Answer: 1. Which of the three halogen acids is the most stable? Least 
stable ? 

2. In what ways are these acids alike? Different? 

PHOSPHATES — ARSENIC — ANTIMONY — BISMUTH 

(Practical Chemistry, pp. 346-358, §§ 419-442) 

Experiment 165 — Tests for Orthophosphoric Acid and 
Orthophosphates 

Materials. — Solutions of disodium phosphate, silver nitrate, ammo¬ 
nium molybdate, ammonium chloride, magnesium sulphate, and 
orthophosphoric acid ; bone ash, fertilizer. 

a. To 5 cc. of disodium phosphate solution add a little silver nitrate 
solution. Observe and describe the result. What is the name and 
formula of the precipitate? 

b. To 5 cc. of disodium phosphate solution add 1 or 2 cc. of dilute 
nitric acid, and an equal volume of ammonium molybdate solution. 
Observe and describe the result. Warm, if no precipitate appears. 
The precipitate is ammonium-phospho-molybdate ((NH 4 ) 3 P0 4 . 
12M0O3, approximately). 

Apply this test to a dilute solution of orthophosphoric acid (in¬ 
stead of disodium phosphate), and state the result. 

c. To magnesium sulphate solution add successively solutions of 
ammonium chloride, ammonium hydroxide, and disodium phosphate. 
Observe and describe the result. The precipitate is ammonium mag¬ 
nesium phosphate. 

d. Shake a little bone ash with warm dilute nitric acid, filter, and 
apply the ammonium molybdate test to the filtrate. State the result. 

Experiment 166 — Preparation of Phosphate Fertilizer 

Materials. — Powdered phosphate rock, concentrated sulphuric acid, 
ammonium molybdate solution. 

Put about 10 gm. of powdered phosphate rock in an evaporating 
dish, add 5 cc. of water, 5 cc. of concentrated sulphuric acid, and mix 
well. Heat gently about ten minutes, stirring frequently. Add 


132 EXPERIMENTS IN PRACTICAL CHEMISTRY 


io to 15 cc. of water, stir, let the mixture settle, and filter. Test 
the filtrate for a phosphate. State the result. 

Experiment 167 — Test for Arsenic 

See Exp. hi d. Write the equation. 

Experiment 168 — Test for Antimony 

See Exp. me. Write the equation. 

Experiment 169 — Test for Bismuth 

Add considerable water to 10 cc. of bismuth trichloride solution. 
The precipitate is bismuth oxychloride. Describe it. What is its 
formula ? 

Experiment 170 — Fusible Alloys 

a. Slip a thin piece of fusible alloy into a test tube half full of 
water, hold a thermometer in the water, heat the water gradually, 
and note the temperature at which the alloy melts. State the result. 

b. Optional. Heat a fusible link or a sprinkler head in water and 
note the temperature at which the alloy melts. State the result. 

SODIUM AND POTASSIUM 

(Practical Chemistry, pp. 360-374, §§ 443-469) 

Experiment 171 — Properties of Sodium 

Caution. — See Exp. 21. 

a. Examine a small piece of sodium, and observe its most obvious 
physical properties, e.g. color, luster, whether hard or soft. 

b. Perform, recall, or repeat (if necessary) the experiment on the 
Interaction of Sodium and Water (Exp. 21). 

c. Fill a dish nearly full of water. Put a piece of sodium on a 
piece of filter paper (a little smaller than the dish), lay the paper upon 
the water, and stand back and observe the result. Wait for the 
slight explosion which usually occurs soon after the action stops. 
Describe all you have seen. What burned? To what is the vivid 
color of the flame probably due ? 

Experiment 172 — Tests for Sodium 

Materials. — Sodium compounds, solutions of potassium hydroxide and 
tartar emetic. 


SODIUM AND POTASSIUM 


133 


a. Apply the flame test to several sodium compounds, using a 
clean test wire in each case (Fig. 89, left). State each result. 

b. Make a solution of a sodium compound slightly alkaline with 
potassium hydroxide solution, and to 10 cc. add a little freshly 
prepared tartar emetic solution. The white precipitate is acid so¬ 
dium pyroantimonate (H 2 Na2Sb 2 0 7 ). 

Experiment 173 — Properties of Sodium Chloride 

Materials. — Sodium chloride (several varieties). 

a. Prepare about 50 cc. of a nearly saturated sodium chloride solu¬ 
tion, and proceed with the crystallization as in Exp. 40. Examine 
and describe the best crystals. 

b. Heat a few crystals of sodium chloride in a test tube. State 
and explain the result. 

c. Put a little sodium chloride ( e.g . table salt) in a test tube, and 
cork the test tube tightly. Put some of the same sample of salt in 
an open dish. Place both where they will not be disturbed for a day 
or two, and then compare the two specimens. State and explain 
the result. 

Experiment 174 — Sodium Carbonate — LeBlanc Process 

Materials. — Sodium sulphate, calcium carbonate, wood charcoal, cal¬ 
cium hydroxide solution. 

Apparatus. — Iron crucible. 

Mix and grind together in a mortar 6 gm. of sodium sulphate, 
4 gm. of powdered calcium carbonate, and 1 gm. of powdered wood 
charcoal. Fuse the whole mixture in an iron crucible or a portion on 
a platinum foil. When cool, heat with a little water and filter. 

Apply the flame test for sodium to a little of the filtrate and state 
the result. Divide the filtrate into two parts. To (1) add 5 cc. of 
dilute hydrochloric acid and to (2) add 5 cc. of calcium hydroxide 
solution. Observe and explain each result. 

Experiment 175 — Hydrolysis of Sodium Carbonate 

Test a solution of sodium carbonate with litmus paper (both kinds), 
and state the result. Interpret by the ionization theory. 

Experiment 176 — Sodium Bicarbonate 

Materials. — Ammonium carbonate, ammonium hydroxide, sodium chlo¬ 
ride. 

Apparatus. — Carbon dioxide generator (see Fig. 68). 


134 EXPERIMENTS IN PRACTICAL CHEMISTRY 


I. Preparation. — Put 8 gm. of powdered ammonium carbonate 
and 75 cc. of ammonium hydroxide into a bottle; add about 35 gm. 
of fine sodium chloride, cork the bottle, and shake the mixture vigor¬ 
ously until most of the solid has dissolved. Pour off the clear solu¬ 
tion into the bottle C. 

Construct a carbon dioxide generator (see Exp. 120) like that 
shown in Fig. 68. Put about 20 gm. of marble in the generator 
bottle A , introduce dilute hydrochloric acid as usual, and pass carbon 
dioxide (free from hydrochloric acid) slowly through the solution in 
the bottle C from thirty to forty-five minutes (or less, if a precipitate 
forms). Then remove the generator, cork the bottle C, and let it 
stand an hour or more to allow the sodium bicarbonate to settle out 
of the solution. Filter, and wash quickly with a very little cold 
water. Dry the precipitate between filter paper. (Note. — If 
only a little of the precipitate is formed, use sodium bicarbonate from 
the laboratory bottle for II.) 

II. Properties. — a. Subject small portions of the precipitate to 
the flame test for sodium and the usual test for a carbonate. State 
the result. 

b. Put a little on moist litmus paper (both colors). Observe and 
explain the result. 

c. Heat a little in a test tube inclined so that the open end is the 
lower. Observe the result. What is the visible product? Apply 
the usual test for carbon dioxide to the gas in the test tube; state 
the result. Continue to heat until there is no further evidence of 
change. Determine what the final residue is by applying to it tests 
for sodium, a bicarbonate as in a and b, and sodium carbonate ( e.g . 
litmus test). State the result. 

Experiment 177 — Properties of Sodium Hydroxide 

a. Perform, recall, or repeat (if necessary) experiments with sodium 
hydroxide which show the effect of (1) exposing it to the air, (2) add¬ 
ing acid to it, (3) dissolving it in water, (4) heating its solution with 
aluminium. 

b. Heat a small piece of sodium hydroxide on a piece of porcelain, 
and describe the result. 

c. Expose a little pulverized sodium hydroxide in a dish to the 
air for a day or more. Describe the final product. Test it for a 
carbonate, and state the result. 

d. Fuse a small quantity of sodium hydroxide on a piece of porce¬ 
lain, add a part of a match stick or a small piece of paper, and con¬ 
tinue the fusion. State the effect on the wood or paper. 


SODIUM AND POTASSIUM 


135 


Experiment 178 — Sodium Hydroxide by Electrolysis 

(Demonstration Experiment) 

Proceed as in Exp. 61. See Fig. 43. 

Experiment 179 — Properties of Borax 

a. Let a piece of red litmus paper stand in borax solution for about 
ten minutes. Observe and explain the result. 

b. Test borax for water of crystallization, and state the result. 
Expose borax crystals to the air for an hour and state the result. 

c. Apply the flame test to a little borax on the end of a clean test 
wire. What element is contained in borax according to this test ? 

d. Dissolve a little borax in water, add 5 cc. of ethyl alcohol, 5 cc. 
of concentrated sulphuric acid, and mix well. Test for borax by 
dipping a clean test wire into the solution and holding it in the outer 
part of the Bunsen flame. Note the color of the flame. 

Experiment 180 — Tests with Borax Beads 

Materials. — Powdered borax, cobalt nitrate, copper sulphate, and man¬ 
ganese sulphate solutions. 

Heat the looped end of a clean test wire and dip it into powdered 
borax. Heat the adhering borax in the flame, rotating the wire 
slowly, until no further change is apparent; continue to dip it into 
the borax and heat in the flame until a small bead is formed. 

a. Cobalt Compounds. — Moisten a borax bead with cobalt nitrate 
solution. Heat the bead in the oxidizing part of the Bunsen flame 



(Fig. 89 left); rotate the bead while heating it. Observe the color 
of the cold bead. If it is black, melt a little more borax into the 
bead; if faintly colored, moisten again with the cobalt solution. The 
color is readily detected by looking at the bead against a white object 
in a strong light, or by examining it with a lens. 













136 EXPERIMENTS IN PRACTICAL CHEMISTRY 


When the color has been definitely determined, heat the bead in 
the reducing flame (Fig. 89 right). Compare the color of the cold 
bead with the previous observation. State the result. 

Note. —The bead may be removed from the wire by dipping it, while 
hot, into water and then rubbing or scraping it from the wire. 

b. Copper Compounds. — Proceed as in a with another bead and 
copper sulphate solution. Compare the colors of the cold beads, 
and state the result. 

c. Manganese Compounds. — Proceed as in a with another bead 
and manganese sulphate solution. Compare the colors of the cold 
beads, and state the result. 

Experiment 181 — Properties of Potassium 

(Demonstration Experiment) 

Caution. — Observe the same precaution as in using sodium. (See 
Exp. 21.) 

a. Examine a small piece of freshly cut potassium, and observe 
its most obvious physical properties. 

b. Proceed as in Exp. 32 b. What compound of potassium is in 
solution? Write the equation. 

Experiment 182 — Tests for Potassium 

Materials. — Potassium compounds, sodium cobaltinitrite solution. 

a. Apply the flame test to several potassium compounds, using a 
clean test wire in each case. State the result. 

b. Add 5 cc. of sodium cobaltinitrite solution to 10 cc. of a mod¬ 
erately concentrated solution of a potassium compound, and shake 
well. The yellow precipitate is potassium cobaltinitrite (K3Co(N02)e) • 

Experiment 183 — Potassium Nitrate 

Materials. — Sodium nitrate, potassium chloride, charcoal. 

I. Preparation. — Dissolve about 15 gm. of potassium chloride 
in about 40 cc. of water, warming if necessary. Add about 17 gm. 
of sodium nitrate, and stir well. Boil several minutes, or until a 
white solid separates. Let the solid settle somewhat, then pour off 
the liquid into an evaporating dish and let it stand till crystals sep¬ 
arate. Pour off the liquid from the crystals. Dissolve the crystals 


CALCIUM — STRONTIUM — BARIUM 


137 


in a small volume of hot water and let the solid crystallize out again. 
Drain off the water and dry the crystals between filter paper. 

II. Properties. — a. Prepare a solution of the final crystals and 
test portions for (1) potassium and (2) a nitrate. State the result. 

b. Test the solution also for (1) sodium and (2) a chloride. State 
the result. Explain it. 

c. Proceed as in Exp. 9 a. 


CALCIUM — STRONTIUM — BARIUM 

(Practical Chemistry, pp. 376-388, §§ 470-486) 

Experiment 184 — Properties of Calcium Carbonate 

a. Put a drop or two of dilute hydrochloric acid on one or more 
specimens of calcium carbonate. State and explain the result. 

b. Attach a small lump of marble to a test wire or lay it on a wire 
gauze, and heat it intensely for ten or fifteen minutes. Test it for 
a carbonate and state the result. What is the name of the solid 
product? Write the equation. 

c. Add 5 cc. of sodium carbonate solution to 5 cc. of calcium chlo¬ 
ride solution. Describe the precipitate. What is it? Write the 
equation. 


Experiment 185 — Tests for Calcium 

Materials. — Calcium compounds, ammonium oxalate and sodium car¬ 
bonate solutions. 

a. Apply the flame test to several calcium compounds, using a 
clean test wire in each case. What is the color of the flame? 

b. Add an excess of ammonium oxalate solution to calcium chloride 
solution, and state the result. The precipitate is calcium oxalate. Di¬ 
vide it into two parts. To (1) add an excess of dilute hydrochloric 
acid, warm gently, and state the final result. To (2) add consider¬ 
able acetic acid and warm gently; observe and state the final result. 
Compare with (1). 

c. Add an excess of sodium carbonate solution to calcium chloride 
solution, and state the result. The precipitate is calcium carbonate. 
Divide it into two parts, and treat with the acids as in b. State the 
results and compare with b. 

d. Devise a test for calcium in calcium carbonate and calcium 
sulphate. Submit the details to the Teacher before proceeding. 


138 EXPERIMENTS IN PRACTICAL CHEMISTRY 

Experiment 186 — Testing Substances of Calcium 

Materials. — Mortar, plaster, bone ash, plaster of Paris, tooth powder, 
whiting, cement, bleaching powder. 

a. Prepare a solution by boiling a little of each substance with 
dilute hydrochloric acid (or dilute nitric acid) and filtering. Test 
the filtrate for calcium by Exp. 185 b (or by the flame test). State 
each result. 

b. Test “ unknowns ” for calcium. 

Experiment 187 — Calcium Oxide and Calcium Hydroxide 

I. Preparation. — a. Proceed as in Exp. 184 b. Let the residue 
cool, put it in an evaporating dish, and add a little water. Observe 
the result. Test the liquid with red litmus paper; apply the flame 
test for calcium. State the results. What calcium compound was 
formed by heating calcium carbonate? By treating the product 
with water? Write each equation. 

b. Prepare calcium hydroxide by adding water slowly to a lump 
of lime, and save it for III. 

II. Properties of Calcium Oxide. — a. Put a lump of fresh cal¬ 
cium oxide on a glass plate or block of wood and let it remain exposed 
to the air for a few days. Examine it at intervals and describe it. 
Describe the final product. What is it ? 

b. What is the result of mixing calcium oxide and water ? Write 
the equation. 

III. Properties of Calcium Hydroxide. —■ a. Add a little solid 
calcium hydroxide to a test tube half full of water and shake 
vigorously. Let the suspended solid settle somewhat, and filter. 
Pour half of the filtrate into an evaporating dish and evaporate it to 
dryness; save the other half. (Meanwhile b may be performed.) 
When evaporated, compare the amount of residue in the dish with 
the amount of solid originally shaken with water. Draw a conclu¬ 
sion regarding the solubility of calcium hydroxide in water. 

b. Taste cautiously of the solution saved from a, and describe the 
taste. Determine the reaction toward litmus; is the solution acid, 
alkaline, or neutral? Is the reaction marked? Heat the solution 
slowly to boiling, and describe the result. What is the effect of in¬ 
creased heat on the solubility of calcium hydroxide in water? 

c. State the result of (1) exposing calcium hydroxide solution to 
the air, and (2) exhaling the breath through calcium hydroxide so¬ 
lution. Express each reaction by an equation. 


CALCIUM — STRONTIUM — BARIUM 


139 


Experiment 188 — Mortar 

Materials. — Lime, sand, old mortar or plaster. 

Apparatus. — Bottle fitted with cork. 

a. Prepare slaked lime by adding hot water slowly to about 30 gm. 
of lime. Add just enough water to make a stiff paste. Add about 
50 gm. of sand, more water if necessary, and mix well. Divide into 
three portions. Spread one portion upon a piece of brick, press an¬ 
other piece of brick upon it, and let the whole remain undisturbed for 
several days. State the final result. 

b. Spread another portion in a thin layer on a board or a glass 
plate, and let it remain as in a. Test it finally for a carbonate and 
state the result. 

c. Put the third portion in a bottle and ©ork tightly. In a day or 
two test as in b. Compare the results of b and c. 

d. Test a lump of old mortar or plaster for a carbonate and state 
the result. 

Experiment 189 — Properties of Cement 

a. Mix a little cement with enough water to form a thick paste 
and spread the paste in a thin layer on a block of wood or a glass 
plate. Let it remain undisturbed for a day 
or more, then examine, describe, and explain. 

b. Prepare two paper cylinders by rolling 
a sheet of paper around a test tube. Close 
one end by folding over the edges of the 
paper. Fill an evaporating dish nearly half 
full of cement, add about the same bulk of 
sand, and mix well. Add water and stir 
until a soft paste is formed. Pour half the 
mixture into each paper cylinder and slip an 
elastic band over the upper end to hold the 
paper in place. Lower one cylinder into a bottle of water and the 
other into an empty bottle (Fig. 90). Let both stand for a day or 
two. Then remove, unroll the paper, and compare the contents. 
State the result. What property of cement is shown by this experi¬ 
ment? 



(left), in water 
(right) 


Experiment 190 — Analysis of Cement 

Materials. — Cement, solutions for c and d. 

a. Preparation of Sample.—Put about 1 gm. of cement in an 
evaporating dish, add concentrated hydrochloric acid, and heat (in 









140 


EXPERIMENTS IN PRACTICAL CHEMISTRY 


the hood) until the cement dissolves. (Filter, if not clear.) Then 
evaporate to dryness, add a little dilute hydrochloric acid and 25 cc. 
of water, and warm gently. Filter and wash the precipitate with a 
little water. Save the precipitate for b and the filtrate for c. 

b. Silica. — Test the precipitate for silica by Exp. 156. State 
the result. 

c. Aluminium and Iron. — To the filtrate from a add ammonium 
hydroxide to alkaline reaction, warm, and filter. Save this filtrate 
for d. Proceed with the precipitate as in (1) and (2). 

(1) Dissolve a portion of the precipitate in sodium hydroxide 
solution and add ammonium chloride solution; the precipitate is 
aluminium hydroxide. Describe it. 

(2) Dissolve another portion in dilute hydrochloric acid, add a 
little concentrated nitric ^cid, and boil. Cool and add a little potas¬ 
sium sulphocyanate solution; the red color of the liquid is due to 
ferric sulphocyanate, and its formation is a test for iron. 

d. Calcium. — To the filtrate from c add ammonium chloride 
solution, ammonium hydroxide, and then considerable ammonium 
oxalate solution. State the result. 

Experiment 191 — Calcium Compounds and Hardness of Water 

Materials. — Calcium hydroxide, solutions of soap, calcium sulphate, 
sodium carbonate, and borax. 

Apparatus. — Carbon dioxide generator (see Fig. 68). 

a. Temporary Hardness. — Prepare a solution of acid calcium 
carbonate by passing carbon dioxide into a mixture of 25 cc. of satu¬ 
rated calcium hydroxide'and 25 cc. of water (distilled or good quality) 
until the precipitate is formed and redissolved (see Exp. 121). 

(1) To 15 cc. of the clear acid calcium carbonate solution add 5 cc. 
of soap solution. Shake well and observe the result. Describe the 
product. Rub some between the fingers and describe the result. 

(2) Boil vigorously 15 cc. of acid calcium carbonate solution for a 
few minutes, filter, and add 5 cc. of soap solution. Shake well and 
observe the result. Compare the results of (2) and (1). 

(3) To 10 cc. of clear acid calcium carbonate solution add 5 cc. 
of saturated calcium hydroxide, shake, filter, and to the clear filtrate 
add 5 cc. of soap solution. Shake well and observe the result. Com¬ 
pare the results of (3), (2), and (1). 

b. Permanent Hardness. — (1) Proceed as in a (1), using 15 cc. 
of calcium sulphate solution (instead of acid calcium carbonate so¬ 
lution). Compare the results of b (1) and a ( 1 )- 


CALCIUM — STRONTIUM — BARIUM 


141 

(2) Boil 15 cc. of calcium sulphate solution, add 5 cc. of soap so¬ 
lution, and shake. Compare the results of b (2), b (1), and a (2). 

(3) To 15 cc. of calcium sulphate solution add 10 cc. of sodium 
carbonate solution, filter, add 5 cc. of soap solution, and shake well. 
Compare the results of b (3) and b (2). 

c. Optional. Try the effect of (1) ammonium hydroxide (in ex¬ 
cess, as told by the odor), and (2) borax solution on both temporarily 
and permanently hard water. 


Experiment 192 — Plaster of Paris 

Materials. — Plaster of Paris, vaseline. 

Mix a little plaster of Paris with enough water to form a thick 
paste. Put the paste on a block of wood or a glass plate. Rub a very 
little vaseline on one side of a coin, and press the coin, coated side 
down, into the paste. Let it stand undisturbed for fifteen or more 
minutes. Then remove the coin carefully, and examine and de¬ 
scribe the effect on the hardened plaster. 


Experiment 193 — Tests for Strontium and Barium 

Materials. — Strontium compounds, calcium sulphate solution; ba¬ 
rium compounds, potassium dichromate solution, acetic acid. 

A. Strontium. — a. Apply the flame test to strontium nitrate and 
other available strontium compounds, using a clean test wire in each 
case. How is the flame colored? Compare with the color pro¬ 
duced by calcium compounds. 

b. To the solution of a strontium compound add calcium sulphate 
solution. The precipitate is strontium sulphate. Write the 
equation. 

B. Barium. — a. Proceed as in A a, using barium nitrate and other 
available barium compounds. 

b. Add dilute sulphuric acid to barium chloride solution (or the 
solution of any barium compound). The precipitate is barium sul¬ 
phate. Describe it. Test it's solubility by heating a little of the 
precipitate in concentrated hydrochloric acid. State the result. 

c. Add potassium dichromate solution to barium nitrate solution. 
The precipitate is barium chromate. Describe it. Test its solu¬ 
bility by heating some of the precipitate separately in acetic acid 
and concentrated hydrochloric acid. State the results. 


142 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 194 — Red Fire and Green Fire 

(Demonstration Experiment) 

Materials. — Strontium nitrate, powdered potassium chlorate, powdered 
shellac, barium nitrate. 

a. Mix carefully small and equal (in bulk) quantities of strontium 
nitrate, potassium chlorate, and shellac on a sheet of paper. Place 
the mixture in an iron pan or on a brick in the hood, and set it afire. 
Describe the result, especially the color. 

b. Proceed as in a, using barium nitrate instead of strontium 
nitrate. 

IRON 

(Practical Chemistry, pp. 391-413, §§ 487-510) 

Experiment 195 — Properties of Iron 

Materials. — Cast and wrought iron, steel; iron wire, thread, and powder; 
special steels. 

Apparatus. — Electric bell and battery, magnet. 

a. Examine typical specimens of cast iron, wrought iron, and steel, 
and state their characteristic physical properties. 

b. Hold a piece of iron wire in the flame for a minute or two. Is 
iron a good conductor of heat? Introduce a piece of iron wire into 
the circuit with an electric bell. Is iron a good conductor of elec¬ 
tricity ? 

c. Determine the specific gravity of a sample of iron and of steel 
by the method given in Exp. 104 b. 

d. Try the action of a magnet on iron and steel. State the result. 

e. Drop a pinch of iron powder into a Bunsen flame. Hold a piece 
of iron thread in the flame. Describe the results, and draw a con¬ 
clusion. 

f. Perform, recall, or repeat (if necessary) experiments which 
show the action of heated iron and (1) oxygen, (2) chlorine, (3) nitro¬ 
gen, (4) nitrous oxide, and (5) sulphur. State each result. 

g. As in f, experiments showing the action of acids with iron. 
State the results. 

h. Test the hardness of (1) different varieties of steel and (2) spe¬ 
cial steels by striking them with a hammer. 

Experiment 196 — Analysis of Slag 

Pulverize a sample of slag (or use mineral wool) and test it for 
(1) silica (Exp. 156) and (2) calcium. State each result. 


IRON 


143 


Experiment 197 — Tests for Ferrous Compounds 

Materials. — Iron powder (or filings), solutions of sodium hydroxide and 
potassium ferricyanide. 

Put 1 or 2 gm. of iron in a test tube, add about 10 cc. of dilute hy¬ 
drochloric acid, and warm gently; ferrous chloride is formed (in 
solution). Proceed at once with the tests. 

(1) Pour a little ferrous chloride into a test tube one-third full 
of sodium hydroxide solution and shake. The precipitate is ferrous 
hydroxide. Note the color. Shake, and describe the changes in 
color. 

(2) Add 5 cc. of ferrous chloride to 5 cc. of potassium/emcyanide 
solution. The precipitate is ferrous ferricyanide. Note the color. 

Experiment 198 — Tests for Ferric Compounds 

Materials. — Solutions of ferric chloride, sodium hydroxide, potassium 
sulphocyanate, and potassium ferrocyanide. 

(1) Add 5 cc. of sodium hydroxide solution to 5 cc. of ferric chlo¬ 
ride solution. The precipitate is ferric hydroxide. Note the color. 

(2) To 5 cc. of ferric chloride add 5 cc. of potassium /errocyanide 
solution. The precipitate is ferric ferrocyanide. Note the color. 

(3) Add 5 cc. of potassium sulphocyanate solution to 5 cc. of 
ferric chloride solution. The wine-red colored solution is caused by 
soluble ferric sulphocyanate. This test readily distinguishes ferric 
from ferrous compounds. 

Experiment 199 — Reduction and Oxidation of Iron 
Compounds 

Materials. — Ferric chloride solution, zinc, ferrous sulphate, potassium 
chlorate. 

a. Put a piece of zinc in ferric chloride solution made slightly 
acid by hydrochloric acid. After the operation has proceeded for 
about fifteen minutes, test separate portions of the solution for a 
ferrous and a ferric compound by Exps. 197 (2) and 198 (3). State 
and explain the results. 

b. (1) To a solution prepared from fresh, or freshly washed, fer¬ 
rous sulphate add a little hydrochloric acid, warm gently, and then 
add a few crystals of potassium chlorate. After heating a short time, 
test separate portions of the solution for a ferric and ferrous com¬ 
pound (as in a). State and explain the results. 


144 EXPERIMENTS IN PRACTICAL CHEMISTRY 


(2) Add 10 cc. of concentrated nitric acid, drop by drop, to a hot 
solution of ferrous sulphate to which a little sulphuric acid has been 
added, and boil. Test and explain as in (1). 

Experiment 200 — Hydrolysis of Ferric Chloride 

Test ferric chloride solution with litmus paper (both kinds). State 
and explain the result. Compare with Exp. 175. 

Experiment 201 — Testing for Iron 

Materials. — Clay, brick, flower pot, bauxite, rusty rock, rouge, sheet 
tin, iron rust, bluing, solutions of potassium ferricyanide and potas¬ 
sium sulphocyanate. 

a. Prepare a solution of the solids by boiling a little of the pow¬ 
dered material with concentrated hydrochloric acid. Test the clear 
solution for iron, both ferric and ferrous, and state the result in each 
case. 

b. Obtain “ unknowns ” and test them for iron as in a. 

c. Add considerable sodium hydroxide solution to a dilute solu¬ 
tion of bluing. Describe and explain the result. 

ALUMINIUM 

(Practical Chemistry, pp. 415-424, §§ 511-524) 

Experiment 202 — Properties of Aluminium 

a. Proceed with aluminium as in Exp. 195 b, c, d. 

b. Warm a piece of aluminium with concentrated hydrochloric 
acid. Test the escaping gas with a blazing joss stick. What is the 
gas ? What compound of aluminium is formed ? 

c. Boil a piece of aluminium with concentrated sodium hydroxide 
solution. Test as in b. Answer the questions in b. 

Experiment 203 — Aluminium Hydroxide 

Materials. —- Solutions of aluminium sulphate, ammonium hydroxide, 
sodium hydroxide, potassium hydroxide, ammonium sulphide, and 
sodium carbonate. 

I. Preparation. — a. Add ammonium hydroxide to a solution 
of aluminium sulphate, and shake well. The precipitate is alumin¬ 
ium hydroxide ; save it for II. 


ALUMINIUM 


H5 

b. Proceed as in a, using aluminium sulphate solution and a very 
little sodium hydroxide solution. Compare-with the result in a. 
Save this precipitate for II. 

II. Properties.— a. Examine the precipitate from I a and note 
its properties, e.g. color, texture, etc. Remove a little and rub it 
between the fingers ; describe the result. 

b. To the precipitate from I b add sodium hydroxide slowly and 
shake constantly until the precipitate dissolves. What aluminium 
compound is formed? 

c. To a portion of the precipitate from I a add considerable ammo¬ 
nium hydroxide, and shake well. Compare with the result in II b. 

d. Add dilute hydrochloric acid to a portion of the precipitate from 
I a, and shake well. State the result. Proceed similarly with other 
acids, e.g. sulphuric and acetic. State the results. 

Experiment 204 — Clarification of Water 

See Exp. 26 c. 

Experiment 205 — Thermit (Demonstration Experiment) 

Materials. —- Thermit, granulated aluminium, barium dioxide, magnesium 
ribbon. 

Apparatus. — Sand crucible 10 cm. (4 in.) deep, brick, sand, iron pan. 

Caution. — Perform this experiment carefully. The molten metal 
may spatter. 

Fill an iron pan with sand and stand it on a brick. Bury the cruci¬ 
ble about halfway in the sand; a box of sand should be near by in 
case the crucible should break. 

Put about 30 gm. of thermit in the crucible. Prepare a fuse mix¬ 
ture by mixing thoroughly about 5 gm. of barium dioxide and 0.5 
gm. of granulated aluminium. Make a hole in the top of the thermit 
and pour in the fuse mixture; insert a piece of magnesium ribbon 
into the heap of fuse mixture. Light the magnesium with the Bunsen 
flame, and stand aside immediately. The reaction is vigorous. De¬ 
scribe it. 

When the crucible is cool, break it open and examine the contents. 
Describe the two parts. What is the name of each? 

Experiment 206 — Tests for Aluminium 

Materials. — Aluminium sulphate, cobaltous nitrate solution, charcoal, 
a. Proceed as in Exp. 203 I a, using an aluminium solution. 


146 EXPERIMENTS IN PRACTICAL CHEMISTRY 


b. To a portion of the aluminium solution add a little sodium 
hydroxide solution and then an excess. To another portion add an 
excess of ammonium hydroxide. Note each result. 

c. Heat a little aluminium sulphate (or any other aluminium com¬ 
pound) on charcoal in the blowpipe flame (oxidizing — see Exp. 
134 B). Cool, and moisten with a drop or two of cobaltous nitrate 
solution. Heat again, and note the color of the residue. 


Experiment 207 — Preparation and Properties of Alum 

Materials. — Aluminium sulphate, potassium sulphate. 

I. Preparation. — Mix 8 gm. of aluminium sulphate and 4 gm. 

of potassium sulphate, and dissolve 
the mixture in about 50 cc. of hot 
water. Pour the solution into dish or 
beaker (Fig. 91) and set it aside to 
crystallize; well-formed crystals may 
be obtained upon a thread suspended 
in the solution. (Meanwhile proceed 
with II a, etc.). Crystals of potassium 
alum will be deposited. Remove the 
best ones; dry and examine. De¬ 
scribe them, giving color, luster, size, 
and crystal form. 

II. Properties. — a. Test a solution 
Fig. 91. — Crystallizing alum of alum separately for aluminium and 

sulphate ions, and state the result. 
Cautiously taste the solution, and describe the result. 

b. Test alum for water of crystallization, and state the result. 

c. Select several good crystals from those prepared in I and ex¬ 
amine them carefully. Describe them. Test as in II, and state the 
results. Allow some crystals to remain exposed to the air for several 
hours. Compare finally with the original crystals. Explain the 
difference. 



Experiment 208 — Aluminium Salts as Mordants 

Materials. -— Solutions of alum, cochineal, and aluminium acetate; aliz¬ 
arin paste, cotton cloth. 

a. Add a little alum solution to a dilute solution of cochineal, then 
add ammonium hydroxide and shake well. Filter, and compare the 
colors of the filtrate and precipitate. 












COPPER 


147 


b. Boil two small pieces of cotton cloth for several minutes 
thoroughly in water. Remove the excess of water. (1) Put one 
piece in a dish or beaker, add 50 cc. of water and 5 cc. of alizarin 
paste, and heat nearly to the boiling point for about two minutes. 
Wash the cloth in water, dry, and then examine. (2) Now proceed 
in the same way with a piece of cotton cloth which has been previously 
mordanted by boiling for about two minutes in aluminium acetate so¬ 
lution. Compare the two pieces of cloth. Explain. 

Experiment 209 — Hydrolysis of Aluminium Salts 

Test a solution of aluminium sulphate and of alum with litmus 
paper. State and explain each result. Compare with Exds. 17 c 
and 200. 

COPPER 

(Practical Chemistry, pp. 426-437, §§ 525-527) 

Experiment 210 — Properties of Copper 

Apparatus. — Electric bell and battery, magnet. 

a. Proceed with copper as in Exp. 195, b, c, d. 

b. Heat a piece of copper wire in the flame until it burns. Note 
the color. What compound is formed? 

c. What is the effect of dilute nitric acid on copper? 

Experiment 211 — Tests for Copper 

Materials. — Copper wire, copper sulphate solution, ammonium hydrox¬ 
ide, acetic acid, potassium ferrocyanide solution. 

a. Heat a copper wire, or a copper compound in the Bunsen flame, 
and observe the color imparted to the flame. 

b. Add considerable ammonium hydroxide to copper sulphate 
solution, shake well, and observe the result. The formation of the 
blue solution is the usual test for copper. 

c. Add to a test tube one-fourth full of water an equal volume of 
copper sulphate solution, and shake ; then add a few drops of acetic 
acid and of potassium ferrocyanide solution. The brown precipitate 
is cupric ferrocyanide (Cu2Fe(CN)e). 

Experiment 212 — Properties of Copper Sulphate 

a. Examine a typical specimen of crystallized copper sulphate, 
and state its characteristic properties. See also Exps. 42, 43. 


148 EXPERIMENTS IN PRACTICAL CHEMISTRY 


b. Let red and blue litmus paper remain in copper sulphate solu¬ 
tion for fifteen minutes or more. State and explain the result. Com¬ 
pare Exps. 175, 200, 209. 

Experiment 213 — Tests for Copper in Alloys 

Materials. —Brass, aluminium bronze, German silver, American cent, 
nickel, and dime. 

a. Prepare a solution of one of the alloys enumerated above by 
boiling a small piece in dilute nitric acid; it may be necessary to treat 
the alloy with several portions of acid. Filter the final liquid if it 
is not clear. Apply the test for copper to the clear solution as in 
Exp. 211 b. Be sure to add an excess of ammonium hydroxide and 
shake well. State the result in each case. 

b. Proceed as in a with “ unknowns” and with metallic substances 
suspected to contain copper, e.g. pins and inexpensive jewelry. 

Experiment 214 — Displacement of Metals — Copper 

Materials. — Copper wire, iron nail, zinc, copper sulphate solution, mer¬ 
curic chloride solution (Poison). 

a. Put a clean copper wire in a test tube half full of mercuric chlo¬ 
ride solution (Poison). After a short time remove the wire and wipe 
it with a soft cloth or paper. Observe and explain the change. 

b. Put a clean iron nail in a test tube half full of copper sulphate 
solution. After a short time remove the nail and examine it. What 
is the deposit ? Explain its formation. 

c. Repeat b, using a strip of zinc instead of an iron nail. Observe 
and explain the result. 

Required Exercise. — Arrange the metals (used in this experiment) in 
the order of their displacing power with reference to copper. 

MAGNESIUM — ZINC — MERCURY 
(Practical Chemistry, pp. 439-45°* §§ 538-560) 

Experiment 215 — Properties of Magnesium and Zinc 

a. Proceed with magnesium and zinc as in Exp. 195 b, c, d. 

b. Perform, recall, or repeat (if necessary) experiments showing 
the results of heating magnesium and zinc (1) in a limited supply of 
air and (2) in an abundance of air; and also treating magnesium and 
zinc with acids. State the results. 


MAGNESIUM — ZINC — MERCURY 


149 


Experiment 216 — Tests for Magnesium 

Materials. — Solutions of magnesium sulphate, ammonium chloride, 
ammonium hydroxide, discdium phosphate. 

a. To a solution of a magnesium compound, e.g. magnesium sul¬ 
phate, add successively solutions of ammonium chloride, ammonium 
hydroxide, and disodium phosphate. A precipitate of ammonium 
magnesium phosphate (NH 4 MgP 0 4 ) is formed. Describe it. 

b. Heat a little magnesium sulphate on charcoal, in a blowpipe 
flame, as in Exp. 206 c. Note the color of the residue. Compare 
with Exp. 206 c. 

Experiment 217 — Testing for Magnesium 

Materials. — Magnesia (“85 per cent”), substances as in b. 

a. Boil a gram or two of “ 85 per cent magnesia ” pipe covering 
with dilute hydrochloric acid. Filter and test the filtrate (diluted) 
for magnesium. State the result. 

b. Proceed as in a with (1) magnesia, (2) milk of magnesia, 
(3) flashlight powder, (4) Epsom salts, (5) magnesite. State each result. 

Experiment 218 — Tests for Zinc 

Materials. — Zinc, zinc sulphate and cobalt nitrate solutions, zinc oxide, 
blowpipe, charcoal. 

a. Apply tests for metallic zinc (see Exp. 215). 

b. Add a very little sodium hydroxide solution to a solution 
of a zinc compound, e.g. zinc sulphate, and shake well. Describe 
the precipitate. What is it? Divide the mixture into three parts. 
(1) To one add considerable sodium hydroxide, (2) to another add 
ammonium hydroxide, and (3) to the third add dilute hydrochloric 
acid. Shake each well, and observe the result. What is the name 
and formula of the zinc compound formed in (1) and (3) ? 

c. Proceed as in Exp. 206 c, using zinc oxide (or any other zinc 
compound). Note the color on the charcoal. Compare with Exps. 
206 c, 216 b. 

d. Add hydrogen sulphide water to zinc sulphate solution and 
note the color of the precipitate. What is the name of the precipitate ? 
Write the equation. 

Experiment 219 — Zinc Hydroxide 

Materials. — Solutions of zinc sulphate, ammonium hydroxide, sodium 
hydroxide, potassium hydroxide, ammonium sulphide, and sodium 
carbonate. 


150 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Proceed as in Exp. 203, using zinc sulphate instead of aluminium 
sulphate. Compare the behavior of aluminium and zinc hydroxides 
when treated with ammonium hydroxide. 


Experiment 220 — Properties of Mercury 

Material. — Mercury. 

a. Pour a drop or two of mercury into an evaporating dish. Ex¬ 
amine the mercury, and state its characteristic properties. Agitate 
the dish, and describe the result. 

b. Stand a funnel in a test tube and carefully pour the mercury 
from the dish into the test tube. Remove the funnel. Heat the 
bottom of the test tube gently and observe the result, especially the 
deposit, if any, upon the upper part of the tube. Scrape a little out 
of the tube with a glass rod. What is the deposit ? What property 
of mercury is shown by this experiment ? 

c. Suggest a method of determining the specific gravity of mer¬ 
cury. If approved by the Teacher, try it. 


Experiment 221 — Mercurous and Mercuric Compounds 

Materials.' —Solutions of mercurous nitrate, mercuric chloride (Poison), 
and stannous chloride. 

I. Mercurous. — a. Add a few drops of hydrochloric acid to a 
little mercurous nitrate solution. The precipitate is mercurous chlo¬ 
ride. Describe it. Note its insolubility in water and in dilute hydro¬ 
chloric acid. Add an excess of ammonium hydroxide. The black 
precipitate is a test for mercury in mercurous compounds. 

b. Add potassium iodide solution to mercurous nitrate solution. 
Describe the result. Give the name and formula of the mercury 
compound formed. Write the equation. 

II. Mercuric. — a. Add a few drops of hydrochloric acid to a 
little mercuric nitrate solution. Compare with the result in I a. Add 
a few drops of ammonium hydroxide, or enough to produce a de¬ 
cided change. Compare with I b. The precipitate is mercuric am¬ 
monium chloride. 

b. Proceed as in I b, using mercuric chloride solution (Poison). 
Compare the results. Give the name and formula of the mercury 
compound formed. Write the equation. 

c. Add a little stannous chloride solution to mercuric chloride and 
note the result; then add considerable stannous chloride solution 


TIN — LEAD 


I 5 i 

and note the change. Write equations for the reactions. (Note. 
— This is the usual test for mercuric compounds). 

Experiment 222 — Displacement of Metals — Magnesium, 
Zinc, and Mercury 

Proceed as in Exp. 214, using these metals and solutions of several 
metallic compounds, e.g. copper sulphate, lead nitrate, silver nitrate, 
and stannous chloride. Try also other metals and solutions of salts 
of magnesium, zinc, and mercury. Note each result and prepare a 
table showing the displacing power of the metals. (Compare Exp. 
214.) 


TIN —LEAD 

(Practical Chemistry, pp. 452-462, §§ 561-578) 

Experiment 223 — Properties of Tin and Lead 

a. Proceed with tin and lead as in Exp. 195 b, c, d. 

b. Bend a piece of tin and note the crackling noise. 

c. Heat a small piece of tin in a test tube with concentrated hydro¬ 
chloric acid in the hood until most of the tin disappears. Stannous 
chloride is formed. Save this solution for Exp. 224. 

d. Add a small piece of tin to a test tube one-fourth full of con¬ 
centrated nitric acid in the hood. Stand the test tube in the rack 
as soon as the action begins. The product is metastannic acid. De¬ 
scribe it. Compare the action of nitric acid on tin, copper, and zinc. 

e. Heat a small piece of tin with aqua regia in a test tube in the 
hood. Observe the result. What tin compound is formed ? 

f. Rub a piece of lead on a hard surface, or with the fingers. 
State the result. 


Experiment 224 — Test for Tin 

Materials. — Solutions of stannous chloride and mercuric chloride 
(Poison). , 

Add a few drops of stannous chloride solution (saved from Exp. 
223 c) to mercuric chloride solution. The white precipitate is mer¬ 
curous chloride. Add considerable stannous chloride and warm 
gently. The gray-black precipitate is finely divided mercury. Write 
the equations for both reactions. 


152 EXPERIMENTS IN PRACTICAL CHEMISTRY 


Experiment 225 — Tests for Lead 

Materials. — Lead nitrate and potassium dichromate solutions. 

a. Reduce lead oxide (or other lead compounds) in the blowpipe 
flame. (See Exp. 134 A a.) 

b. Add hydrogen sulphide solution to a solution of a lead com¬ 
pound. Note the color. Give the name and formula of the pre¬ 
cipitate. 

c. Add dilute hydrochloric acid to a little lead nitrate solution 
until precipitation ceases. The insoluble precipitate is lead chloride. 
Boil some of the precipitate with considerable water. Describe the 
action. 

d. Add dilute sulphuric acid to a little lead nitrate solution until 
precipitation ceases. Give the name and formula of the precipitate. 
Observe its properties. Is it soluble in hot water? Try it. 

e. Repeat d, using potassium dichromate solution instead of sul¬ 
phuric acid. Give the name and formula of the precipitate. De¬ 
scribe it, especially the color. 

Experiment 226 — White Lead 

Materials. —- Lead monoxide, acetic acid, white lead. 

Apparatus. — Carbon dioxide generator. 

a. Heat about 15 cc. of acetic acid in a test tube nearly to boiling, 
and add about 5 gm. of lead monoxide in small portions. Meanwhile 
do b. Shake and heat at intervals until most of the solid disappears. 
Then add about 5 cc. of water, and filter, if the liquid is not clear. 
Pass carbon dioxide (free from acid) through the filtrate (see Exp. 
120 and Fig. 68), and note the result. What is the name and formula 
of the product? Filter, and use the precipitate in c. 

b. Test white lead for (1) lead and (2) a carbonate. State the 
results. 

c. Proceed as in b with the precipitate from a. 

Experiment 227 — Displacement of Metals — Tin and Lead 

Proceed as in Exps. 214, 222 using tin and lead with solutions of 
metals. Tabulate the results and compare with similar experiments. 

Experiment 228 — Testing for Lead 

a. Warm thin shavings of solder with dilute nitric acid, filter, and 
test the filtrate for lead. 



SILVER — GOLD 


153 


b. Proceed as in a using one or more of the following: Tea lead, 
type metal, plumbago, shot, bullets, metallic cap of a bottle, “ lead ” 
of a lead pencil, and “ unknowns.” 

c. Apply the (reduction) blowpipe test for lead to white lead, 
red lead, litharge, dry paint, chrome yellow, and “ unknowns.” 

Experiment 229 — Qualitative Analysis of a Solution of Lead, 
Silver, and Mercury (ous) 

. Materials. — Solution containing lead nitrate, silver nitrate, and mer¬ 
curous nitrate; hydrogen sulphide water, potassium dichromate. 

a. To 10 cc. of the solution add dilute hydrochloric acid drop by 
drop until precipitation ceases. Allow the mixture of precipitated 
chlorides to settle, pour off the liquid carefully, add about 15 cc. of 
water, boil, and filter. This operation dissolves the lead chloride. 
Test the filtrate for lead as in b; save the precipitate for c. 

b. To separate portions of the filtrate add hydrogen sulphide 
water and potassium dichromate solution. Note each result. 

c. Wash the precipitate from a with hot water until the wash water 
does not give a test for lead. Then stand the funnel in a clean test 
tube and pour ammonium hydroxide on the mixture of silver and 
mercurous chlorides. This operation dissolves the silver chloride. 
Test the filtrate as in d; save the precipitate for e. 

d. To the filtrate from c add dilute nitric acid to acid reaction and 
shake. The silver compound is precipitated as silver chloride. 

e. The black residue on the paper is a sufficient test for mercury. 
Confirm thus: Pour a little aqua regia (mixture of 3 cc. of concen¬ 
trated hydrochloric acid and 1 cc. of concentrated nitric acid) upon 
the black precipitate; catch the filtrate in a porcelain dish, dilute 
with about 5 cc. of water, and add a clean copper wire; remove the 
wire in a few minutes, wipe gently, and mercury will be seen on the 
wire as a bright silvery coating. 

SILVER — GOLD 

(Practical Chemistry, pp. 464-472, §§ 579 “ 595 ) 

Experiment 230 — Tests for Silver 
Materials. — Silver coin, hydrogen sulphide, silver nitrate solution. 

a. Hold a silver coin at the mouth of a bottle of hydrogen sulphide 
water, and note the change in color. What silver compound is 
formed ? 


154 EXPERIMENTS IN PRACTICAL CHEMISTRY 


b. Add dilute hydrochloric acid to a silver solution, e.g. silver 
nitrate, and shake. Next add considerable ammonium hydroxide 
and shake, and then add dilute nitric acid to acid reaction. The 
precipitation of silver chloride, its solubility in ammonium hydroxide, 
and its reprecipitation by dilute nitric acid constitute the usual test 
for silver. 

Experiment 231 — Displacement of Metals — Silver 

Summarize the results of previous experiments in which silver or 
silver solutions were used. 

Experiment 232 — Cleaning Tarnished Silver 

Materials. — Silver coin, aluminium, sodium carbonate. 

Dissolve io gm. of sodium carbonate in about 50 cc. of water 
and heat to boiling. Put a small piece of aluminium and a tarnished 
silver coin into the solution; have the metals in contact. Remove 
and examine the coin after a few minutes. State the result. 

Experiment 233 — Preparation and Properties of Silver Halides 

Materials. — Solutions of silver nitrate, potassium chloride, potassium 
bromide, potassium iodide, sodium thiosulphate. 

To separate portions of silver nitrate solution add the chloride, 
bromide, and iodide solution. Observe and state the color of each 
precipitate. Filter each separately. 

Test each precipitate separately by (1) exposing a little to the light, 
(2) shaking some with ammonium hydroxide, and (3) shaking some 
with sodium thiosulphate solution. State each result. Compare 
their behavior under the same conditions. 

Experiment 234 — Silver Salts and Photography 

Materials. — Dilute silver nitrate (17 gm. to a liter), sodium chloride (5.8 
gm. to a liter), and sodium thiosulphate solutions — “hypo” (250 gm. 
to a liter); commercial developer or a substitute (see App. § 6, List G). 
Apparatus. — 4 Test tubes (labeled), black paper, 2 plates (preferably lan¬ 
tern slide plates). 

Note. — Owing to the rapid action of silver bromide, silver chloride is 
used. 

a. Add 5 cc. of the silver nitrate solution to 5 cc. of the sodium 
chloride solution, shake gently, and expose the precipitate to the 


CHROMIUM — MANGANESE 


1 55 


light. Examine frequently and note the time needed for a definite 
change in color. 

b. Prepare silver chloride as in a, and add also 5 cc. of the de¬ 
veloper. Expose, and note the time as in a. Compare the times. 

c. Wrap a piece of dark paper around a test tube to protect it 
from the light, and add the three solutions as in b. After half a min¬ 
ute, examine quickly and note the color. Examine again after half 
a minute more. Compare with b. 

d. Prepare silver chloride as in a, add also 5 cc. of “ hypo ” solu¬ 
tion, and shake well. Note the result. 

e. Optional. Try a to d with silver bromide (prepared from dilute 
silver nitrate and potassium bromide solutions) and compare the 
results with a to d. 

f. Demonstration Experiment. Expose two photographic plates 
(preferably lantern slide plates) or films, develop both in the dark 
room with the class, fix one, and later compare both. Make two 
prints from the fixed plate, and develop. Wash one, and later com¬ 
pare the two prints. 

Experiment 235 — Properties of Gold 

Materials. — Gold, chlorine water, stannous chloride solution. 

a. Proceed as in Exp. 62 b. What gold compound is formed? 
Save the liquid for c. 

b. Proceed as in Exp. 67. What gold compound is formed? Save 
the liquid for c. 

c. Heat (in the hood) the solutions from a and b until most of the 
chlorine has been driven off, dilute the final solution with water, and 
then slowly add a little dilute stannous chloride solution. A purple 
(or black) precipitate of finely divided gold is produced. Its forma¬ 
tion is a test for gold. 

CHROMIUM — MANGANESE 

(Practical Chemistry, pp. 474-477, §§ 596-605) 

Experiment 236 — Tests for Chromium 

Materials. — Borax, chrome alum, potassium carbonate, potassium 
nitrate, acetic acid, nitric acid; sodium hydroxide, lead nitrate, and 
potassium dichromate solutions. 

a. Apply the borax bead test to chrome alum or other chromium 
compounds (see Exp. 180). 


156 EXPERIMENTS IN PRACTICAL CHEMISTRY 


b. Mix equal small quantities of potassium carbonate, potassium 
nitrate, and powdered chrome alum, place the mixture on a piece of 
porcelain, hold it with the test tube holder, or stand it on a wire gauze, 
and heat intensely until the mixture fuses. A yellow mass, due to 
the presence of potassium chromate, resuits. 

If the color is not marked, dissolve the mass in water, add acetic 
acid, slowly.at first, and then boil until the carbon dioxide is expelled. 
Add a few drops of lead nitrate solution to a portion, and yellow lead 
chromate is precipitated. (If the precipitate is white, it is lead 
carbonate, and shows that not all the potassium carbonate was decom¬ 
posed, as intended.) 

c. Proceed as in Exp. 225 e, using potassium chromate or dichro¬ 
mate solution. State the result. 

Experiment 237 — Potassium Chromate and Dichromate 

Materials. — Potassium chromate and dichromate, concentrated hydro¬ 
chloric acid, potassium hydroxide solution. 

a. Prepare a dilute solution of potassium chromate and dichro¬ 
mate, and compare the colors. Save for b and c. 

b. Add concentrated hydrochloric acid to 5 cc. of the solution of 
potassium chromate prepared in a, shake well, and observe the change 
in color. Describe it. Compare with the color of the potassium 
dichromate solution. Into what compound has potassium chro¬ 
mate been changed ? 

c. Add potassium hydroxide solution to 5 cc. of the solution of 
potassium dichromate prepared in a until a change of color is pro¬ 
duced. Describe the color. Compare with the potassium chromate 
solution. Into what compound was the potassium dichromate 
changed ? 

d. Add a few drops of concentrated hydrochloric acid to powdered 
potassium chromate and dichromate in separate test tubes. What 
gas is evolved? 

Experiment 238 — Tests for Manganese 

Materials. — Manganese dioxide, potassium carbonate, potassium ni¬ 
trate, ammonium sulphide, manganese sulphate solution, hydrochloric 
acid, acetic acid, ammonium hydroxide. 

a. Apply the borax bead test to manganese dioxide (or any other 
manganese compound — see Exp. 180). 


CHROMIUM — MANGANESE 


157 


b. Fuse on a piece of porcelain (as in Exp. 236 b) a little man¬ 
ganese dioxide mixed with potassium carbonate and potassium nitrate. 
The green color of the mass is due to potassium manganate. 

c. Add ammonium sulphide to manganese sulphate solution. 
The flesh-colored precipitate is manganese sulphide. Compare with 
other sulphides as to color (see Exp. hi). 


APPENDIX 


1 . The Pressure of Water Vapor in millimeters of mercury is: — 


Tem¬ 

Vapor 

Tem¬ 

Vapor 

Tem¬ 

Vapor 

perature 

Pressure 

perature 

Pressure 

perature 

Pressure 

12 

10.5 

17 

14.4 

22 

•19.7 

12.5 

10.8 

17-5 

14.9 

22.5 

20.3 

13 

11.2 

18 

15-4 

23 

20.9 

I 3-5 

11.6 

18.5 

15-9 

23-5 

21.5 

14 

11.9 

19 

16.4 

24 

22.2 

14.5 

12.3 

19-5 

16.9 

24-5 

22.8 

15 

12.7 

20 

17.4 

25 

23.6 

I 5 -S 

i 3 -i 

20.5 

18.0 

25-5 

24-3 

16 

13.6 

21 

18.5 

26 

25.0 

16.5 

14.0 

21.5 

19.1 

26.5 

25-7 


The numbers in the Vapor Pressure columns are the values for a in 
the formula for the reduction of gas volumes (see the author’s Practi¬ 
cal Chemistry, § 74). 

2 . Laboratory Equipment. — These lists include the apparatus, 
chemicals, and supplies needed for the experiments in this book. 
No allowance is made for breakage, duplicate corks and rubber stop¬ 
pers, and extra glass and rubber tubing. 

List A — Individual Outfit. This list includes the articles 
needed by each pupil (see frontispiece). 


1 Blowpipe. 

1 Blowpipe tube. 

1 Beaker, 250 cc. 

5 Bottles, wide mouth, 250 cc. 

1 Bottle, generator, 250 cc. 

1 Bunsen burner. 

1 Cork to fit smaller test tube. 

1 Cork to fit larger test tube. 

1 Crucible and cover, porcelain, 
No. o. 


1 Crucible block, wood, 10 X 10 
X 2.5 cm. with 3 cm. hole in 
center. 

1 Deflagrating spoon. 

1 Evaporating dish, 7 cm. 

1 Flask, Erlenmeyer, 250 cc. 

100 Filter papers, 10 cm. 

1 Forceps, iron. 

1 Funnel, 65 mm. 

4 Glass plates, 10 X 10 cm. 














APPENDIX 


159 


1 Glass plug (see Exp. 55). 

1 Glass rod, 15 cm. 

1 Glass tube, 150 cm. 1 
1 Graduated cylinder, 25 cc. 

1 Iron stand, clamp (medium), 
ring (8 cm.). 

1 Matches (box). 

1 Mortar and pestle, 8 cm. 

1 Pinch-clamp, Mohr’s. 2 
1 Pneumatic trough, complete. 3 

1 Rubber stopper, 23 mm., 1-hole. 4 

2 Rubber stoppers, 23 mm., 2-hole. 4 
1 Rubber tube, 6 mm. (^ in.) diam., 

60 cm. long (for burner). 

1 Rubber tube, ^ in. diam., 15 
cm. long (for connectors). 


1 Rubber tube, pressure (^- in. 
diam.), 15 cm. long (for drop¬ 
ping funnel). 2 

1 Sponge. 

12 Test tubes, 15 X 1.8 cm. (6 X 
f in.) (“small” test tube). 

3 Test tubes, 20 X 2.5 cm. (8X1 
in.) (“large” test tube). 

1 Test tube brush. 

1 Test tube holder. 

1 Test tube rack. 

1 Test wire (see Int. 6, d.). 

1 Thistle tube, straight stem. 2 

1 Triangle. 5 

1 Wire gauze, 10 X 10 cm. 

2 Wooden blocks, 15 X 15 X 2.5 cm. 


List B — Special Apparatus. 
apparatus needed for a class of ten. 
to experiments. 

1 Balance, chemical ( 24 , 51 , 52 , 87 - 

93 , 125 . 

3 Balances, horn pan (as above). 6 
1 Barometer ( 24 , 87 - 91 , etc.). 

4 Beakers, 250 cc. ( 75 ). 

1 Bottle, 750 cc. ( 87 ). 

5 Bottles, 2500 cc. 

4 Burettes, 50 cc. ( 75 ). 

1 Burner, gas ( 131 ). 

3 Chimneys, lamp. 

1 Cork borers, set (Int. § 5 c). 

1 Cylinder, graduated, 1000 cc. 

2 Cylinders, graduated, 500 cc. 

2 Cylinders, graduated, 250 cc. 

2 Cylinders, graduated, 100 cc. 

5 Crucibles, Hessian, 10 cm. deep 

( 11 ). 


This list includes the special 
Numbers in parentheses refer 

5 Crucibles, iron, 60 cc. ( 124 , 146 , 
154 ). 

2 Desiccators (optional) ( 93 ). 

5 Dishes, lead ( 166 , 158 ). 

2 Electric bells ( 196 , etc.). 

4 Electrodes, carbon. 

1 File, round (Int. § 5 c). 

1 File, triangular (Int. § 3 a). 

3 Flasks, Erlenmeyer, 125 cc. ( 87 ). 

1 Hydrometer (heavy) ( 38 , 114 ). 

1 Hydrometer (light) ( 126 , 139 ). 

3 Jars, 30 X 10 cm. ( 89 , 91 ). 

3 Lenses (magnifiers) ( 3 , 40 , 106 ). 

2 Magnets ( 3 , 195 , etc.). 

5 Pans, iron, 10 cm. 

3 Retorts, stoppered, 250 cc. 

( 81 ). 


1 To fit the rubber stoppers. 2 See Exp. 14. The stem of the thistle tube 
should fit the rubber stoppers. 3 Preferable kind is an indurated fiber Keeler 
No. 4 provided with a shallow flower pot 10 cm. in diameter. An agateware 
pan may be used. 4 To fit the larger test tube. This size (about 23 mm.) 
also fits the average 250 cc. Erlenmeyer flask, the 250 cc. generator bottle 
and the 2500 cc. bottle (acid bottle — See List B). 5 To fit porcelain crucible. 

6 A chemical balance costing about twenty-five dollars is sufficiently accu¬ 
rate. Horn pan balances, if carefully counterpoised, give acceptable re¬ 
sults. (Int. § 8). 


i6o 


APPENDIX 


3 Rubber stoppers, i hole (for 125 
cc. Erlenmeyer flask) ( 87 ). 

2 Scales (Int. § 8) (constantly). 

3 Screws, Hofmann ( 24 ). 

3 Thermometers, — io° to ioo° C. 
(frequently). 

5 Tubes, graduated, 100 cc. ( 89 , 

91 ). 


3 Watch glasses, 9 cm. ( 92 , 93 ). 

1 Weights for chemical balance, 
2 mg. to 50 gm. 

3 Weights for horn pan balance, 
2 mg. to 50 gm. 

3 Weights for scales, 5 gm. to 1000 
gm. 

3 Wing-top burners (Int. § 3 b). 


List C — Demonstration Apparatus. This list includes appa¬ 
ratus — not in other lists — needed for the demonstration experi¬ 
ments. Numbers in parentheses refer to experiments. 


1 Babcock apparatus complete 

( 152 ). 

1 Battery ( 49 , 61 , 94 , 96 - 99 , 178 ). 

1 Battery jar, 12 cm. in diam. ( 61 , 

178 ). 

1 Chlorine tube ( 48 ). 

1 Clamp (large — for condenser) 

(28 I). 

1 Condenser, Liebig, complete (28 I). 

2 Electric light bulbs ( 94 , 103 ). 

1 Fire extinguisher ( 17 ). 


1 Flask, 500 cc. ( 16 ). 

1 Funnel, dropping, 100 cc. ( 103 ). 

1 Hofmann apparatus ( 49 , 97 , 98 ). 

1 Jar, oblong ( 103 ). 

1 Platinum tip (optional) ( 22 ). 

1 Platinum wire (optional) ( 22 ). 

1 Siphon of charged water ( 15 ). 

3 Stoppers, rubber, 1 hole, for U- 
tube (22). 

1 Tube, capillary, 8 cm. ( 22 ), 

1 Tube, U-, 10 cm. ( 22 ). 


List D — Chemicals. This list includes the quantities of chemi¬ 
cals needed for a class of ten. Numbers in parentheses refer to ex¬ 
periments. Starred items may be bought of a local dealer. 


Acid, acetic 

250 cc. 

chloride 

50 gm. 

hydrochloric 

5 1 - 

granulated ( 205 ) 

25 gm. 

nitric 

1.5 1. 

lump (202) 

100 gm. 

orthophosphoric 

25 gm. 

sheet 

600 sq. cm. 

oxalic ( 123 ) 

100 gm. 

sulphate 

200 gm. 

pyrogallic ( 55 ) 

50 gm. 

wire 

1 m. 

sulphuric 

2.5 1. 

Ammoniacal liquor 

150 cc. 

Albumin 

25 gm. 

Ammonium carbonate 

150 gm. 

Alcohol, ethyl 1 

1 1. 

chloride 

500 gm. 

methyl 

IOO cc. 

dichromate (102) 

25 gm. 

Alizarin (paste) ( 208 ) 

10 gm. 

hydroxide 

2.5 1. 

Alloys, fusible ( 170 ) 

25 gm. 

molybdate 

25 gm. 

Alum 

200 gm. 

nitrate (86) 

150 gm. 

chromium 

25 gm. 

oxalate 

50 gm. 

Aluminium acetate 

25 gm. 

sulphate 

25 gm. 

bronze ( 213 ) 

25 gm. 

sulphide 

IOO cc. 


1 Denatured alcohol is suitable for many experiments. 




APPENDIX 

l6l 

Aniline (34) 

So cc. 

sheet* 

50 sq. cm. 

Antimony chloride (168) 

25 gm. 

sulphate 

750 gm. 

Arsenic trioxide 

25 gm. 

wire (No. 20)* 

250 gm. 

Asbestos, shredded (24) 

5 gm. 

Cream of tartar* 

25 gm. 

Baking powder (153)* 

250 gm. 

Dextrose. See Glucose 


Barium carbonate (80) 

25 gm. 

Electrosilicon (156) 

25 gm. 

chloride 

150 gm. 

Ether 

250 cc. 

chloride (pure) (71) 

25 gm. 

Ferric chloride 

50 gm. 

dioxide (5, 205) 

25 gm. 

Ferrous sulphate 

100 gm. 

hydroxide (solid) 

25 gm. 

sulphide 

500 gm. 

nitrate 

100 gm. 

Gasolene* 

2.5 1. 

sulphate (135) 

25 gm. 

Gelatin* 

25 gm. 

Bauxite (201) 

50 gm. 

German silver 

25 gm. 

Bismuth chloride 

25 gm. 

Glass wool (24, 156) 

5 gm. 

Bleaching powder* 

250 gm. 

Glycerin 

IOO cc. 

Bone ash 

25 gm. 

Glucose 

150 gm. 

Borax* 

500 gm. 

Gold leaf 

1 bk. 

Brass (213)* 

25 gm. 

Graphite 

250 gm. 

Cadmium nitrate 

25 gm. 

Hydrogen peroxide* 

500 cc. 

Calcite (87) 

100 gm. 

Hydroquinone (234, List G) 15 gm. 

Calcium (76, 91) 

50 gm. 

Iodine 

So gm. 

carbonate (marble)* 

2.5 kg. 

Infusorial earth (156) 

25 gm. 

chloride 

200 gm. 

Iron filings 

50 gm. 

cyanamide (78) 

25 gm. 

powder 

200 gm. 

fluoride 

200 gm. 

thread (steel wool) 

50 gm. 

oxide (lime)* 

500 gm. 

Joss sticks* 

5 Pkg. 

sulphate 

150 gm. 

Kerosene* 

500 cc. 

Camphor (139)* 

25 gm. 

Lead dioxide 

100 gm. 

Carbon disulphide 

500 cc. 

monoxide (litharge)* 

150 gm. 

tetrachloride 

500 cc. 

nitrate 

100 gm. 

Carborundum, lump 

25 gm. 

red (tetroxide)* 

75 gm. 

powder 

25 gm. 

sheet (thin)* 

75 gm. 

Cement* 

1 kg. 

sulphate (135) 

25 gm. 

Chalk (122) 

25 gm. 

tea (21, 228)* 

2500 sq. cm. 

Charcoal, animal 

100 gm. 

white (carbonate)* 

50 gm. 

blocks 

15 blk.- 

Litmus cubes 

5 gm. 

wood (powd.) 

150 gm. 

paper (each color) 

6 sheets 

Chloroform 

IOO cc. 

Magnesium carbonate (217) 25 gm. 

Chrome yellow* 

25 gm. 

chloride 

25 gm. 

Cobalt chloride (cryst.) 

25 gm. 

oxide 

25 gm. 

nitrate 

50 gm. 

powder (51) 

25 gm. 

Cochineal 

1 gm. 

ribbon 

25 gm. 

Copper borings 

200 gm. 

sulphate 

100 gm. 

bromide 

25 gm. 

Manganese dioxide (gra 

n.) 750 gm. 

nitrate 

25 gm. 

dioxide (powd.) 

50 gm. 

oxide (ic) 

100 gm. 

sulphate 

25 gm. 



162 


APPENDIX 


Mercury 

25 gm. 

bicarbonate* 

250 gm : 

chloride (ic) 

25 gm. 

carbonate* 

500 gm. 

nitrate (ous) 

25 gm. 

chloride 

2 kg. 

oxide ( 4 ) 

25 gm. 

chloride (pure) ( 71 ) 

25 gm. 

Mineral wool ( 156 ) 

10 gm. 

citrate {See Fehling’s 


Naphthol (Alpha). .See List G. 25 gm. 

Solution, List G) 

100 gm. 

Nickel chloride 

25 gm. 

cobaltinitrite ( 182 ) See 

List G. 

sulphate 

25 gm. 

dichromate 

25 gm. 

Paraffin wax* 

25 gm. 

hydroxide 

750 gm. 

Phenol-phthalein solution 

150 cc. 

hypochlorite (solution) 

150 cc. 

Phosphorus, yellow 

25 gm. 

nitrate 

500 gm. 

Plaster of Paris* 

150 gm. 

nitrite 

100 gm. 

Potassium 

1 gm. 

peroxide 

25 gm. 

bromide 

100 gm. 

phosphate (disodium) 

25 gm. 

carbonate 

150 %m. 

silicate (solution) 

150 cc. 

chlorate (cryst.) 

250 gm. 

sulphate 

150 gm. 

chlorate (powd.) 

200 gm. 

sulphite 

200 gm. 

chlorate (pure) ( 71 ) 

25 gm. 

thiosulphate (“hypo”) 

300 gm. 

chloride 

200 gm. 

Solder* 

50 gm. 

chromate 

25 gm. 

Stannous chloride. SeeLiSTG. 50 gm. 

dichromate {See also Battery 

Starch* 

250 gm. 

Solution, List G) 

250 gm. 

Strontium nitrate 

50 gm. 

ferricyanide 

50 gm. 

Sugar (cane)* 

500 gm. 

ferrocyanide 

50 gm. 

Sulphur, flowers 

250 gm. 

hydroxide 

150 gm. 

roll 

750 gm. 

iodide 

100 gm. 

Tannin 

25 gm. 

nitrate 

200 gm. 

Tartar emetic 

25 gm. 

nitrite 

50 gm. 

Thermit ( 205 ) 

25 gm. 

perchlorate 

25 gm. 

Tin, granulated ( 83 ) 

100 gm. 

permanganate 

50 gm. 

rod ( 223 ) 

25 gm. 

sulphate 

100 gm. 

Turpentine* 

50 cc. 

sulphocyanate 

25 gm. 

Type metal ( 228 )* 

50 gm. 

Pumice* 

10 gm. 

Water, distilled 

3 b 

Rosin ( 139 )* 

25 gm. 

Whiting ( 122 )* 

25 gm. 

Shellac (powd.)* 

50 gm. 

Zinc chloride 

25 gm. 

Silver nitrate 

50 gm. 

dust (8) 

25 gm. 

sulphate ( 95 ) 

25 gm. 

granulated 

1 kg. 

Soda lime 

250 gm. 

oxide 

25 gm. 

Sodium 

10 gm. 

sheet* 

200 gm. 

acetate ( 142 ) 

25 gm. 

sulphate 

50 gm. 

List E — Miscellaneous Supplies. The quantities are usually 


small. Numbers in parentheses refer to experiments. Household 
ammonia, banana, beans, bluing (201), bullets (228), butter, candle, 
candy, carrot, celery, clay, colored and unbleached cloth, hard and 
soft coal, cotton, cracker, cranberry, fertilizer (165), flash light powder 



APPENDIX 


163 


(217), flour, flowerpot (201), grape juice (73), hair, horn, cast iron 
(195), iron nails, iron ores, iron rust, iron wire (195), wrought iron 
(195), junket tablet (152), karo (13), lard (144), lemon, limestone, 
lye (144), magnesia covering (217), milk of magnesia (217), magnesite 
(217), maple sugar, phosphorus tipped matches, meat, milk, mo¬ 
lasses, old mortar (122), nut butter (151), dry paint (228), (colored) 
paper, peas, phosphate rock (166), plaster (186), plumbago (116), 
potash, potato, quill toothpick, raisins, rice, rusty rock (200), rouge 
(200), sand, shot (228), slag (196), soap, scouring soap, steel (195), 
stove polish, tacks, (wax) taper, thread, tooth powder, turnip, vase¬ 
line, vinegar, yeast cake. 

List F — Emergency Supplies (see Int. § 11). 25 gm. absorbent 

cotton, 12 bandages (5 cm.), blanket, 50 gm. boric acid solution, 
25 gm. camphor solution, 250 gm. carron oil, 12.5 gm. collodion, 1 book 
court plaster, fire extinguisher, 1 pkg. gauze (picric acid), medicine 
dropper, 1 paper pins, sand and scoop, scissors, 1 bottle smelling salts, 
250 gm. sodium bicarbonate, 1 spool thread, 25 gm. vaseline. 

List G — Solutions. The solutions needed for most experi¬ 
ments are approximately 10 per cent. The concentration of special 
solutions is usually given in the directions for the experiments. 
Certain solutions should be made as follows: 

Acetic acid, dilute, 1 vol. to 5 vols. of water. 

Ammonium carbonate. Dissolve 250 gm. in 1000 cc. of water and add 
85 cc. of ammonium hydroxide. 

Ammonium hydroxide, 1 vol. to 3 vols. of water. 

Ammonium molybdate. Dissolve 15 gm. in 100 cc. of water and pour this 
solution into 100 cc. of nitric acid (1 vol. acid to 1 vol. water). 
Ammonium oxalate, 5 per cent. 

Ammonium sulphide, 1 vol. to 1 vol. of water. 

Barium chloride, 5 per cent. Use distilled water or water free from sul¬ 
phates. 

Barium hydroxide, 1 per cent. Use clear solution. 

Battery solution (Grenet). Dissolve 103 gm. of powdered potassium di¬ 
chromate in 1000 cc. of water and slowly add 103 gm. of concentrated 
sulphuric acid with constant stirring. (A storage battery or 
reduced street current is preferable.) 

Calcium hydroxide. See Lime water. 

Chlorine water. Saturate water with the gas. 

Cobaltous nitrate, 5 per cent. 

Cochineal. Grind a little cochineal with water, dilute as desired, and filter. 
Developer (photographic). Dissolve 11.5 gm. of hydroquinone, 38 gm. of 
sodium sulphite, 75 gm. of sodium carbonate, and 2 gm. of potassium 
bromide in 1000 cc. of water. 


164 APPENDIX 

Fehling’s solution. Dissolve 17.3 gm. of copper sulphate (cryst.) in 150 cc. 
of water. Dissolve 173 gm. of sodium citrate and 100 gm. of sodium 
carbonate (anhydrous) in 850 cc. of water. Pour the first solution into 
the second slowly with constant stirring. The final, clear solution 
will keep well. 

Ferric chloride, 5 per cent. 

Ferrous sulphate, 5 per cent. Must be freshly prepared. Keep a few pieces 
of iron in the solution. 

Hydrochloric acid, dilute, 1 vol. to 5 vols. of water. 

Lead salts. Use distilled water or filter. 

Limewater. Slake lime, add considerable water, shake occasionally, and 
siphon off the clear liquid. 

Litmus. As under Cochineal. 

Mercuric chloride, 5 per cent. POISON ! 

Mercurous nitrate, 5 per cent. Add a little mercury. 

Molisch’s solution. Dissolve 10 gm. of alpha-naphthol in 100 cc. of ethyl 
alcohol (95 per cent). 

Nitric acid, dilute, 1 vol. to 5 vols. of water. 

Phenol-phthalein. Dissolve 1 gm. in 100 cc. of alcohol and dilute slightly 
with water. 

Potassium permanganate, 5 per cent. (Add sufficient water to obtain 
“very dilute” solution.) 

Potassium sulphocyanate, 5 per cent. 

Silver nitrate, 5 per cent. Use distilled water (or water free from chlorides). 

Silver sulphate, 0.5 per cent. See Silver nitrate. 

Sodium cobaltinitrite. Dissolve 10 gm. of sodium nitrite in 20 cc. of water; 
dissolve 6 cc. of acetic acid and 1 gm. of cobaltous nitrate in 15 cc. 
of water. Mix these solutions and filter. 

Stannous chloride. Reduce concentrated hydrochloric acid with tin, dilute 
with water, and keep tin in this solution. 

Sulphuric acid, dilute, 1 vol. to 5 vols. of water. Pour the acid slowly into 
the water, stirring constantly. 


INDEX 


(Numbers indicate pages ) 


Accidents, 12; supplies, 163. 

Acid carbonate, 104. 

Acids, 67-71; acetic, 118; carbonic, 
104; composition, 68; halogen, 
131; hydrochloric, 64-66; nitric, 
75-78; orthophosphoric, 131; 
sulphuric, 100-101; sulphurous, 
42 ; test, 67. 

Air, 57-60; carbon dioxide in, 59; 
combustion, 22; heating metal 
in, 20; oxygen in, 57; testing, 
60; water vapor in, 59. 

Alcohol, ethyl, 117-118. 

Alizarin, 147. 

Alloys, copper, 148; fusible, 132. 

Alum, 146; in baking powder, 125. 

Aluminium, 144-147; equivalent 
weight, 85; hydroxide, 1447 in 
cement, 140; mordants, 146; 
salts, test, 125; test, 145. 

Ammonia, 72-75. 

Ammonium carbonate, 75; chloride, 
74; hydroxide, 72; nitrate, 75, 
79; salts, 74, 125. 

Anhydrous compounds, 48. 

Antimony, test, 132. 

Apparatus, lists, 158-160; common, 
Frontispiece. 

Aqua regia, 66. 

Arsenic, test, 132. 

Babcock test, 122. 

Baking powder, 124. 

Balance, 9-11. 

Barium, 141, 142. 

Bases, 67-71; composition, 68; 
test, 68. 

Bismuth, test, 132. 

Bleaching, 63, 99; powder, 63. 

Blowpipe, use, 115. 

Boiling point, water, 40; elevation, 
91; solutions, 91. 

Bone ash, 131. 


Borax, 135; beads, 135, 136. 

Bread, 121. 

Bromides, 129. 

Bromine, 128. 

Bunsen burner, 2, 113; flame, 113. 

Burettes, 70. 

Butter, 121. 

Calcium, carbonate, 137; equiva¬ 
lent weight, 85 ; hydroxide, 138; 
oxide, 138; salts, test, 125; sul¬ 
phate, 140, 141; test, 137. 

Candle flame, 13, 112. 

Carbon, 23 ; 102-103 ; distribution, 
23; fixed, 108; monoxide, 105; 
test, 103; tetrachloride, 120. 

Carbon dioxide, 23-28; and bev¬ 
erages, 26 ; and combustion, 23 ; 
and fermentation, 24; and fire 
extinguishers, 2 7; and plants, 
27; in air, 59; weight of liter, 
80-82. 

Carbohydrate, 120. 

Carbonates, 104; testing, 104. 

Carbonic acid, 104. 

Carborundum, 127. 

Cement, 139; analysis, 139. 

Charcoal, 102. 

Chemical change, 12, 13; and prop¬ 
erties, 13. 

Chemicals, list, 160-162. 

Chlorides, 66; insoluble, 66. 

Chlorine, 60-63 5 and gold, 63; 
bleaching, 61, 63; by electrolysis, 
62 ; water, 38, 50, 63. 

Chromium, test, 141, 155. 

Coal, analysis, 107; gas, hi. 

Cobalt, test, 135. 

College preparatory experiments. 
See Contents. 

Color of ions, 92. 

Combustion and air, 22; and carbon 
dioxide, 23. 



166 


INDEX 


Compound and elements, 16; and 
mixture, 14. 

Concentration and ionization, 93. 

Copper, 14, 147-148; ion, 92; oxi¬ 
dation, 19; oxide, reduction, 33, 
103; oxide, 33; sulphate, 147; 
sulphate, electrolysis, 89-90; 
test, 136, 147. 

Cork boring, 6. 

Crystallization, 46-49. 

Deliquescence, 49. 

Demonstration experiments. See 
Contents. 

Dextrose, 116. 

Displacement of metals, 148, 151, 
I5 2 , 1 54- 

Distillation, water, 38. 

Dyeing, 146-147. 

Efflorescence, 48, 49. 

Elements and compound, 16. 

Electrolysis, chlorine by, 62 ; copper 
sulphate, 89-90; potassium io¬ 
dide, 91; sodium chloride, 62 ; 
sodium sulphate, 90; water, 51. 

Electrolytes, 87. 

Emergency supplies, 163. 

Equipment, laboratory, 158-160. 

Equivalent weight, aluminium, 85; 
calcium, 85; magnesium, 84; 
zinc, 82, 85, 87. 

Etching, 127. 

Ethyl acetate, 119. 

Fat, in milk, 122-124; test, 120.. 

Fermentation and carbon dioxide, 
24. 

Ferric compounds, 143. 

Ferrous compounds, 143. 

Fertilizer, phosphate, 131. 

Filtering, 5. 

Fire extinguishers, 27. 

Flame, blowpipe, 115; Bunsen, 2-3, 
113; candle, 13, 112; gas, 112. 

Flashing point, kerosene, no. 

Food, 120-125. 

Freezing point, water, 40; depres¬ 
sion, 92; solutions, 92. 

Fuels, 106. 

Fusible alloys, 132. 

Gas, coal, m; flame, 112; illu¬ 
minating, in. 


Gases, collecting, 8. 

Gasolene, 109; and water, 43. 

Glass, bending, 4; cutting, 3; 
drawing, 5; etching, 127. 

Gold, 155; and aqua regia, 66; 
and chlorine, 63; test, 155. 

Graphite, 102. 

Green fire, 142. 

Halogen acids, 131. 

Hardness of water, 140. 

Hydrochloric acid, 64-66. 

Hydrogen, 29-34; burning, 31; by 
electrolysis, 51; chloride, 64-66; 
fluoride, 127; from water, 31, 51; 
peroxide, 52; reduction by, 33; 
sulphide, 95-97. 

Hydrolysis, aluminium compounds, 
147; ferric chloride, 144; sodium 
carbonate, 133. 

Hydrometer, using, 45, 101. 

Illuminating gas, m; flame, 112. 

Ink, bleaching, 64. 

Iodides, 130. 

Iodine, 129, 130; and starch, 117; 
test, 130. 

Iodoform, 118. 

Ionization, 87-93; and concentra¬ 
tion, 93. 

Ions, 87-93; colored, 92 ; colorless, 
92. 

Iron, 142-144; and sulphur, 14; 
in cement, 140; oxidation, 22; 
sulphide, 14-16; tests, 142, 143. 

Kerosene, no; flashing point, no. 

Law, constant composition, 52; 
multiple proportions, 54. 

Lead, 151, 152; separation, 153; 
test, 152; white, 152. 

LeBlanc process, 133. 

Magnesium, 14, 148-149; and oxy¬ 
gen, 52; equivalent weight, 84; 
test, 149. 

Manganese, sulphide, 157; test, 
136, 156. 

Manipulation, 2-11. 

Meniscus, 70. 

Mercuric compounds, 150. 



INDEX 


167 


Mercurous compounds, 150. 

Mercury, 150; oxide, 16; separa¬ 
tion, 153; test, 150. 

Metal and air, 20. 

Milk, 12 2-124. 

Mineral matter, food, 121; milk, 124. 

Mixture, 14. 

Mortar, 139. 

Neutralization, 69-71. 

Nitrates, 77; test, 78. 

Nitric acid, 75-78; test, 78. 

Nitric oxide, 78. 

Nitrogen, 56; dioxide, 78; test, 57. 

Nitrous oxide, 79. 

Non-electrolytes, 87. 

Normal carbonate, 104. 

Orthophosphate, 131. 

Orthophosphoric acid, 131. 

Oxidation, 21; blowpipe, 116; 
chromium compounds, 156; cop¬ 
per, 19; iron compounds, 143 ; 
metals, 22. 

Oxygen, 16-22 ; in air, 57 ; in potas¬ 
sium chlorate, 54; in potassium 
perchlorate, 55 ; in water, 50, 51; 
preparation, 16, 17; properties, 
17, 18, 19; weight of liter, 34. 

Phosphates, 125; fertilizer, 131; 
test, 131. 

Photography, 154. 

Plaster of Paris, 141. 

Potassium, 42, 136; chlorate, com¬ 
position, 54; chromate, 156; 
dichromate, 156; iodide, elec¬ 
trolysis, 91; nitrate, 136; perchlo¬ 
rate, composition, 55; test, 42, 
i 36 ; 

Protein, 120-121; in milk, 122. 

Qualitative analysis, 66, 153. 

Quantitative experiments. See 
Contents. 

Red fire, 142. 

Reduction, blowpipe, 115; by alu¬ 
minium, 145; by carbon, 103; by 
hydrogen, 33; copper oxide, 33; 
iron compounds, 143; mercuric 
compounds, 150. 


Safety lamp, 110. 

Salts, 68-72; chemical behavior, 
88; composition, 68; ions, 88; 
preparation, 72. 

Scales, 9-11. 

Silica, in cement, 140. 

Silicates, 125, 126. 

Silicic acid, 126. 

Silicon, dioxide, 125; test, 126. 

Silver, cleaning, 154; halides, 154; 
photography, 154; separation, 
153; test, 153. 

Slag, 142. 

Soap, 119; and hard water, 140. 

Sodium, 132-135; and water, 31, 
41; bicarbonate, 133, 134; car¬ 
bonate, 133; chloride, 133; hy¬ 
droxide, 134; hypochlorite, 64; 
silicate, 125, 126; sulphate, elec¬ 
trolysis, 90; test, 42, 132. 

Solubility, 43-45; chlorides, 66; 
gases, 43; liquids, 43; solids, 
43-45- 

Solutions, 163; boiling point, 91; 
conducting, 87-88; Fehling’s, 164; 
freezing point, 92; list, 163; 
making, 163; Molisch’s, 164; 
saturated, 45; special, 163; su¬ 
persaturated, 50. 

Stannous chloride, 150, 151. 

Starch, 117. 

Steam, 41. 

Strontium, 141, 142. 

Sucrose, 116. 

Sugar, 116. 

Sulphate, test, 101. 

Sulphides, 97-98, 157. 

Sulphur, 13, 93-101; amorphous, 
95; and iron, 14; dioxide, 98-100; 
monoclinic, 95; orthorhombic, 
94; plastic, 95. 

Sulphuric acid, 100-101. 

Sulphurous acid, 42, 99, 100. 

Supersaturated solution, 50. 

Supplies, 158-164; emergency, 163. 

Tartrates, 124. 

Test, acetic acid, 118; acids, 67; 
alloys, 148; aluminium, 145; 
aluminium salts, 125; ammo¬ 
nium salts, 125; Babcock, 122- 
124; barium, 141; bases, 68; 



INDEX 


168 


bismuth, 132; borax beads, 135 ; 
bromide, 129; calcium, 40, 137; 
calcium salts, 125; carbohy¬ 
drates, 120; carbonate, 124; 
carbon dioxide, 13, 23; cement, 
139; chloride, 40, 66, 67; chro¬ 
mium, 141, 155; copper, 136, 

147; dextrose, 116-117; ethyl 
alcohol, 118; fat, 120; gold, 
i 55; hydrochloric acid, 66; hy¬ 
drogen, 30; hydrogen chloride, 
66; hydroxides, 41-42; impure 
water, 39, 40; iodide, 130; iodine, 
130; iron, 143; lead, 66, 152; 
lime compounds, 40; manganese, 
136, 156; mercury, 150; mercury 
(ous), 66, 150; nitrates, 78; 

nitric acid, 78; oxygen, 19; 

phosphate, 125; potassium, 42, 
136; protein, 120-121; silicon, 
126; silver, 66, 153; sodium, 
42, 132 ; sodium hydroxide, 42 ; 
starch, 117; strontium, 141; 
sugar, 116; sulphate, 40, 101; 

sulphuric acid, 101; sulphurous 
acid, 42, 100; tartrates, 124; tin, 
151; zinc, 116, 149. 

Testing, acids, 69; baking powder, 
124; bases, 69; bread, 121; but¬ 
ter, 121; calcium compounds, 
138; carbon, 103; carbonates, 
104, 124; food, 120-125; illu¬ 
minating gas, hi; iron com¬ 
pounds, 144; magnesium com¬ 


pounds, 149; metals, 116; min¬ 
eral matter, 121; salts, 75; 
silicon compounds, 126; water 
in food, 121. 

Test wire, 6. 

Thermit, 145. 

Titration, 70. 

Vapor pressure, 41, 158. 

Vinegar, 119. 

Water, 37-51; and sodium, 31, 
41; boiling point, 40; calcium 
compounds, 40, 140; chemical 
properties, 41; chlorides, 40; 
chlorine, 38, 50, 63; composition, 
50, 51; distillation, 38; elec¬ 
trolysis, 51; freezing point, 40; 
hardness, 140; in food, 37, 121; 
in milk, 122; lime compounds, 
40; of crystallization, 47, 48; 
organic matter, 39; purification, 
37-38; physical properties, 40; 
vapor pressure, 41, 158; solu¬ 
tion, 43-45; sulphates, 40; tests, 
39; vapor, 41; vapor in air, 59. 

Weighing, 9-11. 

Weight of liter, oxygen, 34; carbon 
dioxide, 80-82. 

White lead, 152. 

Zinc, 148, 149 ; and air, 20; equiv¬ 
alent weight, 82, 85, 87; hy¬ 
droxide, 149; test, 149. 










































































































































































































































































































































































































































































































































































































































































